Thermodynamics · Chemistry · MHT CET

Calculate the change in internal energy of the system if work done by the system is 18 joule and absorbs heat 50 joule in a particular reaction.

Identify from following the correct set of thermodynamic conditions for a reaction to be nonspontaneous at all temperatures.

Calculate $\Delta \mathrm{S}_{\text {Iotal }}$ for a certain reaction if $\Delta \mathrm{H}=-150 \mathrm{~kJ}$ and $\Delta \mathrm{S}=32 \mathrm{JK}^{-1}$ at 300 K .

Which from following is an example of both intensive property and state function?

For a certain reaction, $\Delta \mathrm{H}=-210 \mathrm{~kJ}$ and $\Delta \mathrm{S}=-150 \mathrm{~kJ} \mathrm{~K}^{-1}$ Find the temperature so that $\Delta \mathrm{G}=0$.

Calculate $\Delta \mathrm{H}^{\circ}$ for a reaction if $\Delta \mathrm{S}^{\circ}=120 \mathrm{JK}^{-1}$ and $\Delta \mathrm{G}^{\circ}=28000 \mathrm{~J}$

Calculate the work done in joule if 1 mole of ideal gas is compressed from $25 \mathrm{dm}^3$ to $13 \mathrm{dm}^3$ at constant external pressure 4 bar.

Which from following transformations is endothermic in nature?

Calculate the standard enthalpy change for synthesis of ammonia gas from following data.

i. $\quad 2 \mathrm{H}_{2(\mathrm{~g})}+\mathrm{N}_{2(\mathrm{~g})} \longrightarrow \mathrm{N}_2 \mathrm{H}_{4(\mathrm{~g})} ; \Delta_{\mathrm{r}} \mathrm{H}_1^0=95.4 \mathrm{~kJ}$

ii. $\quad \mathrm{N}_2 \mathrm{H}_{4(\mathrm{~g})}+\mathrm{H}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{NH}_{3(\mathrm{~g})}$;$$ \Delta_{\mathrm{t}} \mathrm{H}_2^0=-187.6 \mathrm{~kJ} $$

Identify from following the correct set of thermodynamic conditions for the reaction to be spontaneous below equilibrium temperature.

Calculate work done if 1 mole of an ideal gas expands isothermally from $2 \mathrm{dm}^3$ to $2.8 \mathrm{dm}^3$ against constant external pressure 1 atm .

Which from following reactions is exothermic?

Calculate work done in isothermal reversible expansion of 1 mole ideal gas from initial pressure 10 bar to final pressure 1 bar at 300 K . $\left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$.

Calculate the standard enthalpy change for reaction,

$$ \begin{aligned} & \mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}_{(l)}+3 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{CO}_{2(\mathrm{~g})}+3 \mathrm{H}_2 \mathrm{O}_{(l)} \\ & \text { if } \Delta_{\mathrm{f}} \mathrm{H}^{\circ}\left(\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}\right)=-280 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ & \Delta_{\mathrm{f}} \mathrm{H}^{\circ}\left(\mathrm{CO}_2\right)=-390 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ & \Delta_{\mathrm{f}} \mathrm{H}^{\circ}\left(\mathrm{H}_2 \mathrm{O}\right)=-285 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned} $$

Identify from following reactions that exhibits negative work done.

Calculate the enthalpy of solution of potassium chloride if its $\Delta_{\mathrm{L}} \mathrm{H}=700 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $\Delta_{\text {hyd }} H=-680 \mathrm{~kJ} \mathrm{~mol}^{-1}$

Calculate the change in internal energy of the system if 20 kJ work is done on the system and it releases 10 kJ heat in a particular reaction.

Calculate the work done in joule if 2 moles of an ideal gas expand isothermally from $15.5 \mathrm{dm}^3$ to $20 \mathrm{dm}^3$ at constant pressure 1 atm .

1.8 g water is vapourised by supplying 4 kJ heat at $100^{\circ} \mathrm{C}$. What is the heat of vapourisation of water at same temperature?

Calculate the standard enthalpy change of following reaction

$$ \begin{aligned} & \mathrm{CH}_{4(\mathrm{~g})}+2 \mathrm{O}_{2(\mathrm{~g})} \rightarrow \mathrm{CO}_{2(\mathrm{~g})}+2 \mathrm{H}_2 \mathrm{O}_{(\ell)} \\ & \text { If } \Delta_{\mathrm{f}} \mathrm{H}^{\circ}\left(\mathrm{CH}_4\right)=-75 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ & \Delta_{\mathrm{f}} \mathrm{H}^{\circ}\left(\mathrm{CO}_2\right)=-394 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ & \Delta_{\mathrm{f}} \mathrm{H}^{\circ}\left(\mathrm{H}_2 \mathrm{O}\right)=-286 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned} $$

Calculate standard enthalpy change of reaction

$$ \mathrm{C}_2 \mathrm{H}_{2(\mathrm{~g})}+\frac{5}{2} \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}, \text { if } $$

$$ \begin{aligned} & \Delta_{\mathrm{f}} \mathrm{H}^{\circ}\left(\mathrm{CO}_2\right)=-393 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ & \Delta_{\mathrm{f}} \mathrm{H}^{\circ}\left(\mathrm{H}_2 \mathrm{O}\right)=-286 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ & \Delta_{\mathrm{f}} \mathrm{H}^{\circ}\left(\mathrm{C}_2 \mathrm{H}_2\right)=227 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned} $$

Calculate the change in internal energy of the system if 25 kJ of work done by the system and it absorbs 10 kJ of heat.

Identify from following an example of intensive property?

Calculate the work done in following reaction at $27^{\circ} \mathrm{C}$.

$$ \begin{aligned} & 4 \mathrm{SO}_{2(\mathrm{~g})}+2 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 4 \mathrm{SO}_{3(\mathrm{~g})} \\ & \left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right) \end{aligned} $$

Which of the following set of thermodynamic conditions is true for the reaction to be spontaneous at high temperature?

Find standard enthalpy of formation of ammonia from following reaction.

$$ \mathrm{N}_{2(\mathrm{~g})}+3 \mathrm{H}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{NH}_{3(\mathrm{~g})} ; \Delta_{\mathrm{r}} \mathrm{H}^0=-92.0 \mathrm{~kJ} $$

Calculate work done if 1 mole of an ideal gas compressed isothermally and reversibly from 12 $\mathrm{dm}^3$ to $6 \mathrm{dm}^3$ at $300 \mathrm{~K} .\left[\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right]$

Identify from following physical transformations that exhibits decrease in entropy.

Calculate the standard enthalpy change of following reaction.

$$ \mathrm{C}_2 \mathrm{H}_{4(\mathrm{~g})}+3 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{CO}_{2(\mathrm{~g})}+2 \mathrm{H}_2 \mathrm{O}_{(l)} $$

If $\Delta_{\mathrm{f}} \mathrm{H}^{\circ}\left(\mathrm{C}_2 \mathrm{H}_4\right)=-52 \mathrm{~kJ} \mathrm{~mol}^{-1}$

$$ \begin{aligned} & \Delta_{\mathrm{f}} \mathrm{H}^{\circ}\left(\mathrm{CO}_2\right)=-390 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ & \Delta_{\mathrm{f}} \mathrm{H}^{\circ}\left(\mathrm{H}_2 \mathrm{O}\right)=-286 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned} $$

Which from following process involves zero work done?

Calculate the constant external pressure required to expand 2 moles of an ideal gas from volume $15 \mathrm{dm}^3$ to $20 \mathrm{dm}^3$ if amount of work done is -600 J .

Calculate the enthalpy of vaporisation of ethanol if 11.5 g of ethanol is completely vaporised by supplying 11.8 kJ of heat.

Calculate the enthalpy change of vaporisation of benzene if 13 gram of benzene vaporised by supplying 5.1 kJ of heat.

Calculate the entropy change of surrounding if 2 moles of $\mathrm{H}_2$ and 1 mole of $\mathrm{O}_2$ gas combine to form 2 moles of liquid water by releasing 525 kJ heat to surrounding at constant pressure and at 300 K .

Which of the following reactions exhibits decrease in entropy?

Calculate standard internal energy change for $\mathrm{OF}_{2(\mathrm{~g})}+\mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \longrightarrow 2 \mathrm{HF}_{(\mathrm{g})}+\mathrm{O}_{2(\mathrm{~g})}$ at 300 K , if $\Delta_{\mathrm{f}} \mathrm{H}^{\circ}$ of $\mathrm{OF}_{2(\mathrm{~g})}, \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}$ and $\mathrm{HF}_{(\mathrm{g})}$ are 20, -250 and $-270 \quad \mathrm{~kJ} \mathrm{~mol}^{-1}$ respectively. $\left[\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right]$

Calculate internal energy change of a system if work done by the system is 8 J and heat supplied to it is 40 J .

Which of the following equation relates temperature of a reaction with $\Delta \mathrm{H}^{\circ}$ and $\Delta \mathrm{S}^{\circ}$ at equilibrium?

The enthalpy of vaporisation of a liquid is $30 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and entropy of vaporisation is $75 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$. Calculate boiling point of liquid at 1 atm .

Find work done on 2 mole of an ideal gas at $27^{\circ} \mathrm{C}$ if it is compressed reversibly and isothermally from $5.05 \times 10^6 \mathrm{Nm}^{-2}$ to $1.01 \times 10^5 \mathrm{Nm}^{-2}$ pressure.

A system performs mechanical work equal to 15 kJ and looses 2 kJ of heat to surrounding. What is the change in internal energy of a system?

Find the constant external pressure required to expand a gas from 2.5 L to 4.5 L if amount of work done is 500 J at 298 K ?

In a particular reaction ' x ' kJ of heat is released by the system and ' y ' kJ of work done is done on the system. What is internal energy change?

Calculate the value of $\Delta G$ for the following reaction. $\mathrm{N}_2 \mathrm{O}_{4(\mathrm{~g})} \longrightarrow 2 \mathrm{NO}_{2(\mathrm{~g})}$ if $\Delta \mathrm{H}=57.44 \mathrm{~kJ}$ and $\Delta \mathrm{S}=176 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$.

Under similar conditions enthalpy of freezing is exactly opposite to

100 ml of $\mathrm{H}_{2(\mathrm{~g})}$ and 100 ml of $\mathrm{Cl}_{2(\mathrm{~g})}$ were allowed to react at 1 bar pressure as

$$\mathrm{H}_{2(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{HCl}_{(\mathrm{g})}$$

What will be the PV type of work done during reaction?

Identify the process from following such that volume of system remains constant.

Two moles of an ideal gas are compressed isothermally and reversibly from 40 L to 20 L at 300 K . What is the work done? $\left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$

Calculate the enthalpy change when 12 g carbon react with sufficient hydrogen to form methane. If enthalpy of formation of methane is $-75 \mathrm{~kJ} \mathrm{~mol}^{-1}$.

Which among the following pair of properties are intensive?

2 moles of an ideal gas expands isothermally from $5 \mathrm{dm}^3$ to $10 \mathrm{dm}^3$ at a constant external pressure of 1.5 bar. Calculate work done.

An ideal gas expands against constant external pressure of 2 bar from 5 lit to 8 lit and absorbs 10 kJ of heat. What is $\Delta \mathrm{U}$ of the system?

For an ideal gas, the heat of reaction at constant pressure and heat of reaction at constant volume are related by equation _________

For the reaction $\mathrm{CH}_{4(\mathrm{~g})}+\mathrm{H}_{2(\mathrm{~g})} \longrightarrow \mathrm{C}_2 \mathrm{H}_{6(\mathrm{~g})}$ $\mathrm{K}_{\mathrm{p}}=3.356 \times 10^{17}$, calculate $\Delta \mathrm{G}^{\circ}$ for the reaction at 298 K .

A gas expands isothermally against a constant external pressure of 1 bar from 10 dm$^3$ to 20 dm$^3$ by absorbing 800 J of heat from surrounding. Calculate value of $\Delta$U.

Which of the following equations indicates increase in entropy?

Which from following statements is true about internal energy?

2 moles of an ideal gas are expanded isothermally and reversibly from 20 L to 40 L at 300 K . Calculate work done. ( $\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$).

10 g each of $\mathrm{NH}_3, \mathrm{~N}_2, \mathrm{Cl}_2$ and $\mathrm{H}_2 \mathrm{~S}$ are expanded isothermally and reversibly at same temperature. Identify gas that performs maximum work.

Identify the factor from following on which heat of reaction does not depend.

For the reaction,

$$2 \mathrm{H}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}, \Delta \mathrm{H}^{\circ}=-573.2 \mathrm{~kJ}$$

What is heat of decomposition of water per mol?

For the reaction,

$$\mathrm{C}_3 \mathrm{H}_{8(\mathrm{~g})}+5 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 3 \mathrm{CO}_{2(\mathrm{~g})}+4 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}$$

at constant temperature, $\Delta \mathrm{H}-\Delta \mathrm{U}$ is

What is change in internal energy of the system when work done by the system is 150 J and system release 300 J of heat?

Two moles of an ideal gas is expanded isothermally from a volume of $300 \mathrm{~cm}^3$ to 2.5 $\mathrm{dm}^3$ at 298 K against a constant pressure at 1.9 bar. Calculate the work done in joules.

Calculate heat required to convert 9 g of liquid water to water vapours from following equations.

$$\begin{aligned} & \mathrm{H}_{2(\mathrm{~g})}+\frac{1}{2} \mathrm{O}_{2(\mathrm{~g})} \longrightarrow \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \Delta \mathrm{H}=-57 \mathrm{kCal} \\ & \mathrm{H}_{2(\mathrm{~g})}+\frac{1}{2} \mathrm{O}_{2(\mathrm{~g})} \longrightarrow \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \Delta \mathrm{H}=-68.3 \mathrm{kCal} \end{aligned}$$

One mole of a gas occupying 3 L volume is expanded against a constant external pressure of 1 bar to a volume of 15 L . Calculate work done by the system

Which from the following defines enthalpy of a system?

Which of the following symbols represent heat of reaction at constant volume?

Calculate the entropy change for melting 1 g ice at $0^{\circ} \mathrm{C}$ in $\mathrm{Jg}^{-1} \mathrm{~K}^{-1}$ if heat of fusion of ice at $0^{\circ} \mathrm{C}$ is $80 \mathrm{~J} \mathrm{~K}^{-1}$.

Which of the following set of properties is correct when one mole of a gas is heated keeping volume constant by increasing temperature and supplying 500 J of heat?

Find value of Q from following equations.

(i) $\mathrm{C}_{(\mathrm{s})}+\mathrm{O}_{2(\mathrm{~g})} \longrightarrow \mathrm{CO}_{2(\mathrm{~g})} \Delta \mathrm{H}=\mathrm{QkJ}$

(ii) $\mathrm{C}_{(\mathrm{s})}+\frac{1}{2} \mathrm{O}_{2(8)} \longrightarrow \mathrm{CO}_{2(8)} \Delta \mathrm{H}=-\mathrm{x} \mathrm{kJ}$

(iii) $\mathrm{C}_{(\mathrm{s})}+\frac{1}{2} \mathrm{O}_{2(\mathrm{~s})} \longrightarrow \mathrm{CO}_{2(\mathrm{~g})} \Delta \mathrm{H}=-\mathrm{ykJ}$

Which of the following statements is appropriate as per first law of thermodynamics?

Given that $$\mathrm{C}_{(\mathrm{g})}+4 \mathrm{H}_{(\mathrm{g})} \longrightarrow \mathrm{CH}_{4(\mathrm{g})} \Delta \mathrm{H}^{\circ}=-1665 \mathrm{~kJ}$$

What is bond energy per mole of $\mathrm{C}-\mathrm{H}$ bond?

If bond formation energy of $\mathrm{H}-\mathrm{H}$ bond is $-433 \mathrm{~kJ} \mathrm{~mol}^{-1}$ find the bond dissociation energy for 0.5 mole $H_{2(g)}$.

What is the value of standard enthalpy of formation of dihydrogen?

Calculate Gibbs energy change for a reaction having $\Delta \mathrm{H}=31400 \mathrm{~J}, \Delta \mathrm{~S}=32 \mathrm{~J} \mathrm{~K}^{-1}$ at $1000^{\circ} \mathrm{C}$ ?

If 100 L gas is enclosed in a cylinder, absorbs 302.6 J of heat and expands to 200 L against constant external pressure of 2 atm . Calculate internal energy change of the gas.

Which of the following is true for the value of $\Delta \mathrm{H}-\Delta \mathrm{U}$ at constant volume?

Calculate enthalpy change for following reaction.

$$\mathrm{H}_2 \mathrm{C}=\mathrm{CH}_{2(\mathrm{~g})}+\mathrm{H}_{2(\mathrm{~g})} \longrightarrow \mathrm{H}_3 \mathrm{C}-\mathrm{CH}_{3(\mathrm{~g})}$$

[The bond energy of $\mathrm{C}-\mathrm{H}, \mathrm{C}-\mathrm{C}, \mathrm{C}=\mathrm{C}$ and $\mathrm{H}-\mathrm{H}$ is $414,347,615$ and 435 kJ respectively]

Which among the following is NOT an intensive property?

In a process 605 J heat is absorbed by the system and 380 J work is done by the system on surrounding. What is the value of $\Delta$U?

A gas absorbs certain amount of heat and expands by $200 \mathrm{~cm}^3$ against a constant external pressure of $2 \times 10^5 \mathrm{Nm}^{-2}$. What is work done by system?

For a reaction $$\mathrm{A}+\mathrm{B} \rightarrow$$ products $$\Delta \mathrm{H}$$ is $$-84.2 \mathrm{~kJ}$$ and $$\Delta \mathrm{S}$$ is $$-200 \mathrm{~J} \mathrm{~K}^{-1}$$. Calculate the highest value of temperature so that the reaction will proceed in forward direction.

Which from following thermodynamic properties is a path function?

Calculate the PV type of work for the following reaction at 1 bar pressure.

$$\mathrm{\mathop {{C_3}{H_{6(g)}}}\limits_{(150\,mL)} + \mathop {HC{l_{(g)}}}\limits_{(150\,mL)} \buildrel {} \over \longrightarrow \mathop {{C_3}{H_7}C{l_{(g)}}}\limits_{(150\,mL)}}$$

If enthalpy change for following reaction at $$300 \mathrm{~K}$$ is $$+7 \mathrm{~kJ} \mathrm{~mol}^{-1}$$ find the entropy change of surrounding?

$$\mathrm{H}_2 \mathrm{O}_{(\mathrm{s})} \longrightarrow \mathrm{H}_2 \mathrm{O}_{(\ell)}$$

Calculate $$\Delta \mathrm{H}$$ for following reaction, at $$25{ }^{\circ} \mathrm{C}$$.

$$\mathrm{NH}_2 \mathrm{CN}_{(\mathrm{g})}+\frac{3}{2} \mathrm{O}_{2(\mathrm{~g})} \longrightarrow \mathrm{N}_{2(\mathrm{~g})}+\mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}$$

$$(\Delta \mathrm{U}=-740.5 \mathrm{~kJ}, \mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1})$$

Identify false statement regarding isothermal process from following.

Two moles of an ideal gas expand freely and isothermally from $$5 \mathrm{~dm}^3$$ to $$50 \mathrm{~dm}^3$$. What is the value of $$\Delta H$$ ?

Which among the following is intensive and extensive properties respectively?

An ideal gas absorbs $$210 \mathrm{~J}$$ of heat and undergoes expansion from $$3 \mathrm{~L}$$ to $$6 \mathrm{~L}$$ against a constant external pressure of $$10^5 \mathrm{~Pa}$$. What is the value of $$\Delta U$$ ?

Which of the following processes exhibits increase in internal energy?

One mole of an ideal gas performs $$900 \mathrm{~J}$$ of work on surrounding. If internal energy increases by $$625 \mathrm{~J}$$, find the value of $$\Delta \mathrm{H}$$.

Which of the following temperature values in Fahrenheit $$\left({ }^{\circ} \mathrm{F}\right)$$ is equal to $$50^{\circ} \mathrm{C}$$ ?

Calculate the work done in the following reaction at $$300 \mathrm{~K}$$ and at constant pressure.

$$\left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$$

$$4 \mathrm{HCl}_{(\mathrm{g})}+\mathrm{O}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{Cl}_{2(\mathrm{~g})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}$$

Which among the following is NOT the feature of reversible process?

A gas absorbs $$150 \mathrm{~J}$$ heat and expands by $$300 \mathrm{~cm}^3$$ against a constant external pressure $$2 \times 10^5 \mathrm{~N} \mathrm{~m}^{-2}$$, What is $$\Delta \mathrm{U}$$ of the system?

Equal masses in grams of $$\mathrm{H}_2, \mathrm{~N}_2, \mathrm{Cl}_2$$, and $$\mathrm{O}_2$$, are enclosed in cylinders separately. If these gases expand isothermally and reversibly by $$10 \mathrm{~dm}^3$$ at $$300 \mathrm{~K}$$, the work done by gas is maximum for

If lattice enthalpy and hydration enthalpy of $$\mathrm{KCl}$$ are $$699 \mathrm{~kJ} \mathrm{~mol}^{-1}$$ and $$-681.8 \mathrm{~kJ} \mathrm{~mol}^{-1}$$ respectively. What is the enthalpy of solution of $$\mathrm{KCl}$$ ?

For reaction, $$\mathrm{CO}_{(\mathrm{g})}+\frac{1}{2} \mathrm{O}_{2(\mathrm{~g})} \longrightarrow \mathrm{CO}_{2(\mathrm{~g})}$$

Which of the following equations is CORRECT at constant $$\mathrm{T}$$ and $$\mathrm{P}$$ ?

Calculate amount of methane formed by liberation of $$149.6 \mathrm{~kJ}$$ of heat using following equation.

$$\mathrm{C}_{(\mathrm{s})}+2 \mathrm{H}_{2(\mathrm{~g})} \longrightarrow \mathrm{CH}_{4(\mathrm{~g})} \quad \Delta \mathrm{H}=-74.8 \mathrm{~kJ} / \mathrm{mol}$$

Calculate $$\Delta \mathrm{S}_{\text {total }}$$ for the following reaction at $$300 \mathrm{~K}$$.

$$\mathrm{NH}_4 \mathrm{NO}_{3(\mathrm{~s})} \longrightarrow \mathrm{NH}_{(\mathrm{aq})}^{+}+\mathrm{NO}_{3(\mathrm{aq})}^{-}$$

$$\left(\Delta \mathrm{H}=28.1 \mathrm{~kJ} \mathrm{~mol}^{-1}, \Delta \mathrm{S}_{\mathrm{sys}}=108.7 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$$

What is the work done during oxidation of 4 moles of $$\mathrm{SO}_{2(\mathrm{~g})}$$ to $$\mathrm{SO}_{3(\mathrm{~g})}$$ at $$27^{\circ} \mathrm{C}$$?

$$\left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1(\mathrm{~g})} \mathrm{mol}^{-1}\right)$$

Identify the type of system if boiling water is kept in a half filled closed vessel.

What is the value of increase in internal energy when system does $$8 \mathrm{~J}$$ of work on surrounding by supplying $$40 \mathrm{~J}$$ of heat to it?

Which among the following is TRUE for isobaric process?

What is value of PV type of work for following reaction at 1 bar?

$$\underset{(200 \mathrm{~mL})}{\mathrm{C}_2 \mathrm{H}_{4(\mathrm{~g})}}+\underset{(150 \mathrm{~mL})}{\mathrm{HCl}_{(\mathrm{g})}} \longrightarrow \mathrm{C}_2 \mathrm{H}_5 \mathrm{Cl}_{(\mathrm{g})}$$

A gas absorbs $$200 \mathrm{~J}$$ heat and expands by $$500 \mathrm{~cm}^3$$ against a constant external pressure $$2 \times 10^5 \mathrm{~N} \mathrm{~m}^{-2}$$. What is the change in internal energy?

Which among the following pair of properties is intensive?

If $$8.84 \mathrm{~kJ}$$ heat is liberated for formation of $$3 \mathrm{~g}$$ ethane, calculate its $$\triangle_{\mathrm{f}} \mathrm{H}^{\circ}$$.

The difference between $$\Delta \mathrm{H}$$ and $$\Delta \mathrm{U}$$ is usually significant for systems consisting of :

What is change in internal energy when system releases $$8 \mathrm{~kJ}$$ of heat and performs $$660 \mathrm{~J}$$ of work on the surrounding?

Calculate the final volume when 2 moles of an ideal gas expand from $$3 \mathrm{~dm}^3$$ at constant external pressure 1.6 bar and the work done in the process is $$800 \mathrm{~J}$$.

For $$\mathrm{NaCl}_{(\mathrm{s})}$$ enthalpy of solution is $$4 \mathrm{~kJ} \mathrm{~mol}^{-1}$$ and lattice enthalpy is $$790 \mathrm{~kJ} \mathrm{~mol}^{-1}$$. What is hydration enthalpy of $$\mathrm{NaCl}$$ ?

What is the value of $$\Delta H-\Delta U$$ for the following reaction?

$$2 \mathrm{C}_{(\mathrm{s})}+3 \mathrm{H}_{2(\mathrm{~g})} \rightarrow \mathrm{C}_2 \mathrm{H}_{6(\mathrm{~g})}$$

An ideal gas expands by $$1.5 \mathrm{~L}$$ against a constant external pressure of $$2 \mathrm{~atm}$$ at $$298 \mathrm{~K}$$. Calculate the work done?

Which among the following reactions exhibits $$\Delta \mathrm{H}=\Delta \mathrm{U}$$ ?

An ideal gas expands by performing $$200 \mathrm{~J}$$ of work, during this internal energy increases by $$432 \mathrm{~J}$$. What is enthalpy change?

Calculate the value of $$\Delta G$$ for following reaction at $$300 \mathrm{~K}$$.

$$\begin{aligned} & \mathrm{H}_2 \mathrm{O}_{(\mathrm{s})} \longrightarrow \mathrm{H}_2 \mathrm{O}_{(l)} \\ & \left(\Delta \mathrm{H}=7 \mathrm{~kJ}, \Delta \mathrm{S}=24.8 \mathrm{~J} \mathrm{~K}^{-1}\right) \end{aligned}$$

What is the value of temperature in degree Celsius at absolute zero ?

Calculate the work done when 2 moles of an ideal gas expand from a volume of $$5 \mathrm{~dm}^3$$ to $$7 \times 10^{-3} \mathrm{~m}^3$$ against a constant external pressure of $$2.02 \times 10^5 \mathrm{~Nm}^{-2}$$ ?

What is the heat of formation of $$\mathrm{HCl}_{(\mathrm{g})}$$ from following equation?

$$\mathrm{H}_{2(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{g})} \rightarrow 2 \mathrm{HCl}_{(\mathrm{g})} \Delta_{\mathrm{f}} \mathrm{H}=-194 \mathrm{~kJ}$$

If $$\mathrm{Q}$$ is the heat liberated from the system and $$\mathrm{W}$$ is the work done on the system then first law of thermodynamics can be written as,

For isochoric process, the first law of thermodynamics can be expressed as

When certain volume of gas expands against a constant external pressure of $$2.40 \times 10^5 \mathrm{~Pa}$$ at 300 $$\mathrm{K}$$ to $$2.2 \times 10^{-3} \mathrm{~m}^3$$. If the work obtained is $$-0.048 \mathrm{~kJ}$$. What is the initial volume of the gas?

What is internal energy change when $$62 \mathrm{~J}$$ of work is done on the system and $$128 \mathrm{~J}$$ of heat is transferred to surrounding?

A gas is allowed to expand against a constant external pressure of 2.5 bar from an initial volume 'x' L to final volume of 4.5 L. If amount of work done is 5 dm$$^3$$ bar, what is the value of 'x'?

In a process, a system performs $$238 \mathrm{~J}$$ of work on it's surrounding by absorbing $$54 \mathrm{~J}$$ of heat. What is the change in internal energy of system during this operation?

When $$\mathrm{x} \mathrm{kJ}$$ heat is provided to a system, work equivalent to $$\mathrm{y} \mathrm{J}$$ is done on it. What is internal energy change during this operation?

What is the constant external pressure of an ideal gas when expanded from $$2 \times 10^{-2} \mathrm{~m}^3$$ to $$3 \times 10^{-2} \mathrm{~m}^3$$, if the work done by the gas is $$-5.09 \mathrm{~kJ}$$ ?

During a process, system absorbs $$710 \mathrm{~J}$$ of heat and increases the internal energy by $$460 \mathrm{~J}$$. What is the work performed by system?

Which among the following is NOT an intensive property?

A system gives out $$\mathrm{x} \mathrm{~J}$$ of heat and does $$\mathrm{y} \mathrm{~J}$$ of work on it's surrounding. What is the internal energy change?

A system does 394 J of work on surrounding by absorbing 701 J heat. What is the change in internal energy of the system?

Formation of $$\mathrm{NO}_{2(\mathrm{g})}$$ from $$\mathrm{N}_{2(\mathrm{g})}$$ and $$\mathrm{O}_{2(\mathrm{g})}$$ is an endothermic process. Which of the following is true for this reaction?

What is enthalpy of formation of $$\mathrm{NH}_3$$ if bond enthalpies are as $$(\mathrm{N} \equiv \mathrm{N})=941 \mathrm{~kJ},(\mathrm{H}-\mathrm{H})=436 \mathrm{~kJ},(\mathrm{N}-\mathrm{H})=389 \mathrm{~kJ}$$ ?

What is the difference between $$\Delta H$$ and $$\Delta \mathrm{U}$$ for reaction given below at $$298 \mathrm{~K}$$ ?

($$\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$$

$$2 \mathrm{C}_6 \mathrm{H}_{6(\ell)}+15 \mathrm{O}_{2(\mathrm{~g})} \rightarrow 12 \mathrm{CO}_{2(\mathrm{~g})}+6 \mathrm{H}_2 \mathrm{O}_{(\ell)}$$

Enthalpy of formation of methane is $$-$$75 kJ/mol. What is the enthalpy change for formation of 24 g of methane?

The expansion of gas having no opposing force is called as

1 mole of an ideal gas expands isothermally and reversibly by decreasing pressure form $$210 \mathrm{~kPa}$$ to $$105 \mathrm{~kPa}$$ at $$300 \mathrm{~K}$$. What is the work done? $$\left(\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)$$

When 1 mole of gas is heated at constant volume, the temperature rises form $$273 \mathrm{~K}$$ to $$546 \mathrm{~K}$$. If heat supplied to the gas is $$\mathrm{x~J}$$, then find the correct statement from following.

What is the value of $$\mathrm{\Delta H-\Delta U}$$ for the formation of 2 moles of ammonia from $$\mathrm{H_{2(g)}}$$ and $$\mathrm{N_{2(g)}}$$ ?

Two moles of an ideal gas are expanded isothermally from $$15 \mathrm{dm}^3$$ to $$20 \mathrm{dm}^3$$. If the amount of work done is $$-6 \mathrm{dm}^{-3}$$ bar, find external pressure needed to obtain this work.

Find the value of $$-197^\circ$$C temperature in Kelvin.

Which among the following is NOT an extensive property?

A gas is allowed to expand in an insulated container against a constant external pressure of 2.5 atm from $$2.5 \mathrm{~L}$$ to $$4.5 \mathrm{~L}$$, the change in internal energy of the gas in joules is

What is the work done when a gas is compressed from 2.5 $$\times$$ 10$$^{-2}$$ m$$^3$$ to 1.3 $$\times$$ 10$$^{-2}$$ m$$^3$$ at constant external pressure of 4.05 bar?

Calculate heat of formation of $$\mathrm{HCl}$$ gas from following reaction.

$$\mathrm{H}_{2(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{HCl}_{(\mathrm{g})} ; \Delta \mathrm{H}=-194 \mathrm{~kJ}$$

Calculate difference between $$\Delta \mathrm{H}$$ and $$\Delta \mathrm{U}$$ for following reaction at $$25^{\circ} \mathrm{C}$$ ?

$$\mathrm{C}_2 \mathrm{H}_{6(\mathrm{~g})}+3.5 \mathrm{O}_2 \rightarrow 2 \mathrm{CO}_{2(\mathrm{~g})}+3 \mathrm{H}_2 \mathrm{O}_{(l)}\left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$$

The change in internal energy of a system depends upon

Which of the following reactions shows work of compression?

Calculate change in enthalpy when 39 g acetylene is completely burnt with oxygen and enthalpy of combustion of acetylene is $$-$$1300 kJ/mol.

(At. mass C = 12, H = 1)

An ideal gas on isothermal reversible compression from 10L to 5L performs 1730J of work at 300 K. Calculate number of moles of gas involved in compression? (R = 8.314 J K$$^{-1}$$ mol$$^{-1}$$)

What is standard $N \equiv N$ bond enthalpy from following reaction,

$$\begin{aligned} & \mathrm{N}_2(g)+3 \mathrm{H}_2(g) \longrightarrow 2 \mathrm{NH}_3(g) ; \Delta H^{\circ}=-83 \mathrm{~kJ} \\ & \left(\Delta H^{\circ}(\mathrm{H}-\mathrm{H})=435 \mathrm{~kJ} ; \Delta H^{\circ}(\mathrm{N}-\mathrm{H})=389 \mathrm{~kJ}\right) \\ \end{aligned}$$

For the reaction,

$$\mathrm{N}_2(g)+3 \mathrm{H}_2(g) \longrightarrow 2 \mathrm{NH}_3(g) ; \Delta H$$

is equal to

When 6.0 g of graphite reacts with dihydrogen to give methane gas, 37.4 kJ of heat is liberated. What is standard enthalpy of formation of $\mathrm{CH}_4(\mathrm{~g})$ ?

Work done when 2 mole of an ideal gas is compressed from a volume of $$5 \mathrm{~m}^3$$ to $$2.5 \mathrm{~m}^3$$ at 300 K, under a pressure of 100 kpa is

If entropy of a solid is greater than zero, at $$T=0$$, it is called

A sample of gas absorbs $$4000 \mathrm{~kJ}$$ of heat and surrounding does $$2000 \mathrm{~J}$$ of work on sample. What is the value of $$\Delta U$$ ?

If $$38.55 \mathrm{~kJ}$$ of heat is absorbed, when 6.0 of $$\mathrm{O}_2$$ react $$\mathrm{CIF}$$ according to reaction.

$$2 \mathrm{CIF}(g)+\mathrm{O}_2(g) \longrightarrow \mathrm{Cl}_2(g)+\mathrm{OF}_2(g)$$

What is the standard enthalpy of reaction?

An ideal gas expands isothermally and reversibly from $$10 \mathrm{~m}^3$$ to $$20 \mathrm{~m}^3$$ at $$300 \mathrm{~K}$$, performing $$5.187 \mathrm{~kJ}$$ of work on surrounding, calculate number of moles of gas used.

"The mass and energy both are conserved in an isolated system", is the statement of

The temperature of $32^{\circ} \mathrm{C}$ is equivalent to

A gas performs 0.320 kJ work on surrounding and absorbs 120 J of heat from the surrounding. Hence, change in internal energy is

Based on first law of thermodynamics which of the following is correct

Identify the equation in which change in enthalpy is equal to change in internal energy

Two moles of an ideal gas is expanded isothermally and reversibly at 300 K from 1 L to 10 L . The enthalpy change in kJ is

$$\begin{aligned} & \text { If } \mathrm{C}(s)+\mathrm{O}_2(g) \rightarrow \mathrm{CO}_2(g), \Delta H=-X \\ & \mathrm{CO}(g)+\frac{1}{2} \mathrm{O}_2(g) \rightarrow \mathrm{CO}_2(g), \Delta H=-Y \end{aligned}$$ Calculate $\Delta_f H$ for $\mathrm{CO}_{(g)}$ formation

Three moles of an ideal gas are expanded isothermally from a volume of $300 \mathrm{~cm}^3$ to 2.5 L at 300 K against a pressure of 1.9 atm . The work done in joules is

Calculate the difference between heat of combustion of carbon monoxide gas at constant pressure and at constant volume at $27^{\circ} \mathrm{C} ?\left(R=2 \mathrm{cal} \mathrm{K}^{-1} \mathrm{~mol}^{-1}\right)$

For a process, entropy change of a system is expressed as