Electrochemistry · Chemistry · MHT CET
MCQ (Single Correct Answer)
What is percent dissociation of $\mathrm{NH}_4 \mathrm{OH}$ if molar conductance at zero concentration for $\mathrm{NH}_4 \mathrm{Cl}$, NaCl and NaOH are 130, 109 and $213 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ respectively and molar conductivity of $0.01 \quad \mathrm{M} \quad \mathrm{NH}_4 \mathrm{OH}$ is $9.0 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ ?
What is degree of dissociation of $\mathrm{CH}_3 \mathrm{COOH}$ if, $\wedge^{\circ}\left(\mathrm{CH}_3 \mathrm{COO}^{-}\right)=50 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$, $\wedge^{\circ}\left(\mathrm{H}^{+}\right)=350 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ and molar conductivity of $5 \times 10^{-2} \mathrm{M} \mathrm{CH}_3 \mathrm{COOH}$ is $20 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ ?
What is the SI unit of resistivity?
What is reduction potential of hydrogen gas electrode when pure hydrogen gas is at I atmospheric pressure and platinum electrode is in contact with HCl solution of pH 1 at 298 K ?
What happens to the emf for the cell, ${ }^{-} \mathrm{Zn}_{(\mathrm{s})}\left|\mathrm{Zn}_{(1 \mathrm{M})}^{+2} \| \mathrm{Ag}^{+1}(1 \mathrm{M})\right| \mathrm{Ag}_{(\mathrm{s})}^{+}$if concentration of $\mathrm{Ag}^{+1}$ decreases to 0.1 M ?
Which of the following net cell reaction takes place in a galvanic cell containing copper electrode and standard hydrogen electrode?
$$ \mathrm{E}^{o}\left(\mathrm{Cu}_{(\mathrm{aq})}^{+2} \mid \mathrm{Cu}_{(\mathrm{s})}\right)=+0.34 \mathrm{~V} $$
Which of the following changes takes place at positive electrode during recharging of lead accumulator?
For the cell reaction, $\mathrm{A}_{(\mathrm{s})}+\mathrm{B}_{(\mathrm{eq})}^{+_2} \longrightarrow \mathrm{~A}_{(\mathrm{eq})}^{+_2}+\mathrm{B}_{(\mathrm{s})}$ if equilibrium constant of reaction is $10^4$ at 298 K . What is standard emf of cell?
If $\mathrm{E}^{-}\left(\mathrm{Cu}_{(a q)}^{+2} \mid \mathrm{Cu}_{(s)}\right)=+0.34 \mathrm{~V}$. What is potential for $\mathrm{Cu}_{(s)} \rightarrow \mathrm{Cu}_{(\mathrm{aq})}^{+2}(0.1 \mathrm{M})+2 \mathrm{e}^{-}$at 298 K ?
If standard reduction potential $\left(\mathrm{E}^{\circ}\right)$ of $\left(\mathrm{Mg}_{(\mathrm{aq})}^{+2} \mid \mathrm{Mg}_{(\mathrm{s})}\right),\left(\mathrm{Ag}_{(\mathrm{aq})}^{+} \mid \mathrm{Ag}_{(\mathrm{s})}\right),\left(\mathrm{Zn}^{+2}{ }_{(\mathrm{aq})} \mid \mathrm{Zn}_{(\mathrm{s})}\right)$ and $\left(\mathrm{Cu}^{+2}{ }_{(\text {aq })} \mid \mathrm{Cu}_{(\text {s })}\right)$ are $-2.37 \mathrm{~V},+0.79 \mathrm{~V},-0.76 \mathrm{~V}$ and +0.34 V respectively. Which of the following reaction is spontaneous?
What is molar conductivity at zero concentration in $\Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ for aluminium sulphate, if molar ionic conductivities at zero concentration of $\mathrm{Al}^{+3}$ and $\mathrm{SO}_4^{-2}$ are $189 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ and $50.1 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ respectively?
For the cell involving following reaction.
$$ \mathrm{Zn}_{(\mathrm{s})}+\mathrm{Ni}_{(\mathrm{aq})}^{+2} \longrightarrow \mathrm{Zn}_{(\mathrm{aq})}^{+2}+\mathrm{Ni}_{(\mathrm{s})}, \mathrm{E}_{\mathrm{cell}}^*=0.5 \mathrm{~V} . $$
What is standard Gibb's energy change of cell reaction?
If $\mathrm{E}^{\circ}\left(\mathrm{Zn}_{(\mathrm{aq})}^{+2} \mid \mathrm{Zn}_{(\mathrm{s})}\right)=-0.76 \mathrm{~V}$.
Calculate potential for $\mathrm{Zn}_{(\mathrm{s})} \rightarrow \mathrm{Zn}^{+2}(0.01 \mathrm{M})+2 \mathrm{e}^{-}$at 298 K .
Which from following statements is true regarding the cell emf at 298 K for
${ }^{\ominus} \mathrm{Ni}_{(s)}|\stackrel{+2}{\mathrm{~N}} \mathrm{i}(0.01 \mathrm{M}) \| \stackrel{+}{\mathrm{Ag}}(0.01 \mathrm{M})| \stackrel{\oplus}{\mathrm{Ag}_{(s)}}$
The standard emf for cell, ${ }^{\ominus} \mathrm{Cd}_{(\mathrm{s})}\left|{ }^{+2} \mathrm{Cd}(1 \mathrm{M}) \| \stackrel{+2}{\mathrm{Cu}}(1 \mathrm{M})\right| \mathrm{Cu}_{(\mathrm{s})}{ }^{\oplus}$ is 0.74 V .
If concentration of $\mathrm{Cd}_{(\mathrm{aq})}^{+2}$ and $\mathrm{Cu}_{(\mathrm{aq})}^{+2}$ decreases by 10 times at 298 K . Calculate emf of cell.
A hypothetical galvanic cell is ${ }^{\ominus} \mathrm{A}_{(\mathrm{s})} \mid \stackrel{+}{\mathrm{A}}(1 \mathrm{M})\|\stackrel{+2}{\mathrm{~B}}(1 \mathrm{M})\| \stackrel{\oplus}{\mathrm{B}}_{(\mathrm{s})}$ and emf of cell is positive. What is the possible cell reaction?
Consider galvanic cell, ${ }^{\ominus} \mathrm{A}_{(\mathrm{s})}\left|\mathrm{A}_{(\mathrm{aq})}^{+2}\right|\left|\mathrm{B}_{(\mathrm{aq})}^{+}\right| \mathrm{B}_{(\mathrm{s})}^{\oplus}$
if emf of cell is positive, identify a correct cell reaction from following.
Standard potential of electrode reaction $\mathrm{Cu}_{(\mathrm{aq})}^{+2}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Cu}_{(\mathrm{s})}$ is +0.34 V .
What is standard potential of reaction
$$ 2 \mathrm{Cu}_{(\mathrm{s})} \longrightarrow 2 \mathrm{Cu}_{(\mathrm{aq})}^{+2}+4 \mathrm{e}^{-} ? $$
What is value of $E_{\text {cell }}$ at 298 K for the reaction, $\mathrm{Zn}_{(\mathrm{s})}+\mathrm{Cu}^{+2}(0.1 \mathrm{M}) \longrightarrow \mathrm{Zn}^{+2}(0.1 \mathrm{M})+\mathrm{Cu}_{(\mathrm{s})}$ if $\mathrm{E}_{\text {cell }}^{\circ}=1.1 \mathrm{~V}$ ?
$$ \begin{aligned} & \text { If } \mathrm{E}^{\circ}\left(\mathrm{Fe}_{(\mathrm{aq})}^{+2} \mid \mathrm{Fe}_{(\mathrm{s})}\right)=-0.44 \mathrm{~V} \text { and } \\ & \mathrm{E}^{\circ}\left(\mathrm{Sn}_{(\mathrm{aq})}^{+2} \mid \mathrm{Sn}_{(\mathrm{s})}\right)=-0.14 \mathrm{~V} \end{aligned} $$
What is standard emf of cell containing the two electrodes?
If $\mathrm{E}^o{}\left(\mathrm{AI}_{(\mathrm{eq})}^{+3} \mid \mathrm{AI}_{(\mathrm{s})}\right)=-1.66 \mathrm{~V}$. What is potential of $\mathrm{Al}_{(\mathrm{s})} \longrightarrow \mathrm{Al}^{+3}(0 \cdot 1 \mathrm{M})+3 \mathrm{e}^{-}$at 298 K ?
Which of the following reactions exhibit minimum standard reduction potential?
If standard reduction potential $\left(E^{\circ}\right)$ of $\left(\mathrm{Ni}_{(\mathrm{aq})}^{+2} \mid \mathrm{Ni}_{(\mathrm{s})}\right)$ and $\left(\mathrm{Al}_{(\mathrm{aq})}^{+3} \mid \mathrm{Al}_{(\mathrm{s})}\right)$ are -0.25 V and -1.66 V respectively. What is standard emf of cell reaction $2 \mathrm{Al}_{(\mathrm{s})}+3 \mathrm{Ni}_{(\mathrm{aq})}^{+2} \longrightarrow 2 \mathrm{Al}_{(\mathrm{aq})}^{+3}+3 \mathrm{Ni}_{(\mathrm{s})}$
If $\mathrm{E}^{\cdot}\left(\mathrm{Mg}_{(\mathrm{aq})}^{+2} \mid \mathrm{Mg}_{(\mathrm{s})}\right)=-2.37 \mathrm{~V}$. What is potential for $\mathrm{Mg}_{(\mathrm{s})} \longrightarrow \mathrm{Mg}^{+2}(0.01 \mathrm{M})+2 \mathrm{e}^{-}$at 298 K ?
If $\mathrm{E}^{\circ}\left(\mathrm{Ag}^{+}{ }_{(\mathrm{aq})} \mid \mathrm{Ag}_{(\mathrm{s})}\right)=+0.80 \mathrm{~V}$ What is potential developed for $\mathrm{Ag}_{(\mathrm{s})} \longrightarrow \mathrm{Ag}^{+1}(0.01 \mathrm{M})+\mathrm{e}^{-}$at 298 K ?
Which of the following relations about $\mathrm{E}_{\text {cell }}^{\circ}$ is false?
For cell reaction,
$$ 2 \mathrm{Al}_{(\mathrm{s})}+3 \mathrm{Cu}_{(\mathrm{aq})}^{+2} \longrightarrow 2 \mathrm{Al}_{(\mathrm{aq})}^{+3}+3 \mathrm{Cu}_{(\mathrm{s})} $$
If $\Delta \mathrm{G}^{\circ}=-1158 \mathrm{~kJ}$, what is $\mathrm{E}_{\text {cell }}^{\circ}$?
If $\mathrm{E}^*\left(\mathrm{Mg}^{+2}{ }_{(\mathrm{aq})} \mid \mathrm{Mg}_{(\mathrm{s})}\right)=-2.37 \mathrm{~V}$.
What is potential for $\mathrm{Mg}_{(\mathrm{s})} \rightarrow \mathrm{Mg}^{+2}(0.1 \mathrm{M})+2 \mathrm{e^-}$ at 298 K ?
If standard emf of cell $\mathrm{Zn}_{(\mathrm{s})}\left|\mathrm{Zn}_{(\mathrm{iM})}^{+2}\right| \mathrm{Ag}_{(\mathrm{iM})}^{+1} \mid \mathrm{Ag}_{(\mathrm{s})}$ is 1.55 V .
What is electrical work done under standard conditions?
Assume the cell reaction,
$$ \mathrm{A}_{(\mathrm{s})}+\mathrm{B}_{(\mathrm{aq})}^{+2} \longrightarrow \mathrm{~A}_{(\mathrm{aq})}^{+2}+\mathrm{B}_{(\mathrm{s})} $$
if $\Delta \mathrm{G}^{\circ}=-386 \mathrm{~kJ}$ at 298 K . What is $\mathrm{E}_{\mathrm{Cell}}^0$ ?
Which of the following change takes place at positive electrode during working of dry cell?
Which from following statement is correct regarding emf of cell for the cell reaction,
$$ \mathrm{Cd}_{(\mathrm{s})}+\mathrm{Cu}_{(\mathrm{aq})}^{+2} \longrightarrow \mathrm{Cd}_{(\mathrm{aq})}^{+2}+\mathrm{Cu}_{(\mathrm{s})} $$
if concentration of $\mathrm{Cd}^{+2}$ is 10 times greater than concentration of $\mathrm{Cu}_{(\mathrm{aq})}^{+2}$ at 298 K .
Which of the following species acts as reducing agent during working of hydrogen-oxygen fuel cell?
Standard potential $\left(\mathrm{E}^{\circ}\right)$ of $\mathrm{Zn}_{(\mathrm{aq})}^{+2}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Zn}_{(\mathrm{s})}$ is -0.76 V .
What is standard potential of reaction $2 \mathrm{Zn}_{(\mathrm{s})} \longrightarrow 2 \mathrm{Zn}_{(\mathrm{aq})}^{+2}+4 \mathrm{e}^{-}$?
Which from following formulae is used to obtain value of $\mathrm{E}_{\text {cell }}^r$ for a reaction taking place in Dry cell?
For a Galvanic cell consisting zinc electrode and standard hydrogen electrode,
$$ \mathrm{E}^{\mathrm{o}}\left(\mathrm{Zn}_{(\mathrm{aq})}^{+2} \mid \mathrm{Zn}_{(\mathrm{s})}\right)=-0.76 \mathrm{~V} $$
Identify the reaction that takes place at positive electrode during working of cell?
What is the number of faraday required to form $1 \mathrm{~mol} \mathrm{H}_2$ by reduction of $\mathrm{H}^{+}$ions?
For the cell,
${ }^{\ominus} \mathrm{Zn}_{(\mathrm{s})}\left|\mathrm{Zn}^{+2}(1 \mathrm{M})\right|\left|\mathrm{Ag}^{+1}(1 \mathrm{M})\right| \mathrm{Ag}_{(\mathrm{s})}{ }^{\oplus}$
If concentration of $\mathrm{Zn}^{+2}$ decreases to 0.1 M at 298 K , then emf of cell
For the cell reaction,
$$\mathrm{Zn}_{(\mathrm{s})}+2 \mathrm{Ag}_{(\mathrm{aq})}^{+} \longrightarrow \mathrm{Zn}_{(\mathrm{aq})}^{+2}+2 \mathrm{Ag}_{(\mathrm{s})}$$
Cell potential is less than $\mathrm{E}_{\text {cell }}^{\circ}$ by 0.0592 V at 298 K when
Calculate the cell constant of conductivity cell containing 0.1 M KCl solution having resistance $60 \Omega$ and conductivity $0.014 \Omega^{-1} \mathrm{~cm}^{-1}$ at $25^{\circ} \mathrm{C}$.
What is the number of faraday required to produce 0.18 g aluminium at cathode during electrolysis of molten $\mathrm{AlCl}_3$ ? (Molar mass of $\mathrm{Al}=27 \mathrm{~g} \mathrm{~mol}^{-1}$ )
Which from following equations represents a correct relationship between standard cell potential and equilibrium constant for cell reaction?
What is the conductivity of 0.05 M NaOH solution having resistance 31.5 ohm and cell constant $0.315 \mathrm{~cm}^{-1}$ ?
Which from the following concentrations of a weak electrolyte solution exhibits maximum molar conductivity?
Consider the following cell $\mathrm{E}^{\circ}$ cell $=1.007 \mathrm{~V}$ and $\mathrm{E}^{\circ}$ calomel $=0.242 \mathrm{~V}$ What is the standard potential of Zn ?
Calculate the percentage dissociation of 0.05 M solution of weak electrolyte if its molar conductivity and molar conductivity at infinite dilution are respectively. $3.3 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ and $132 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$.
The conductivity of 0.02 M solution of $\mathrm{AgNO}_3$ is $0.00216 \Omega^{-1} \mathrm{~cm}^{-1}$ at 298 K . What is its molar conductivity?
What is the decreasing order of deposition of metal on electrode if standard reduction potentials are given as -
$\mathrm{Ag}^{+}\left|\mathrm{Ag}=0.80 \mathrm{~V}, \mathrm{Cu}^{2+}\right| \mathrm{Cu}=0.337 \mathrm{~V}$
$\mathrm{Sn}^{2+}\left|\mathrm{Sn}=-0.136 \mathrm{~V}, \mathrm{Cd}^{2+}\right| \mathrm{Cd}=-0.403 \mathrm{~V}$
The $\mathrm{E}_{\text {cell }}^{+}$of $\mathrm{Cu}_{(\mathrm{s})}\left|\mathrm{Cu}_{(\mathrm{1M})}^{++} \| \mathrm{Ag}_{(\mathrm{1M})}^{+}\right| \mathrm{Ag}_{(\mathrm{s})}$ is 0.647 volt. Calculate the $\mathrm{E}_{\mathrm{Ag}}^{\circ}$ if $\mathrm{E}_{\mathrm{Cu}}^{\circ}$ is 0.153 V .
Calculate the mass of ' Ca ' deposited at cathode by passing 0.8 ampere current through molten $\mathrm{CaCl}_2$ in 60 minutes. [Molar mass of $\mathrm{Ca}=40 \mathrm{~g} \mathrm{~mol}^{-1}$ ]
What is the concentration of an electrolyte solution to have molar conductivity of $101 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ and conductivity of $1.01 \times 10^{-2} \Omega^{-1} \mathrm{~cm}^{-1}$ at $298 \mathrm{~K} ?$
Cell constant of a conductivity cell is $0.9 \mathrm{~cm}^{-1}$ and resistance shown by $\mathrm{AgNO}_3$ solution is 6530 ohm. What is the conductivity of $\mathrm{AgNO}_3$ solution?
Which of the following cannot be used as standard solution for determination of cell constant of conductivity cell?
When fused NaCl undergoes electrolysis the product formed at cathode is
Which of the following element is used in photoelectric cell?
The resistance of conductivity cell filled with 0.1 M KCl solution is 100 ohm and conductivity is $1.70 \times 10^{-4} \mathrm{~S} \mathrm{~cm}^{-1}$. What is the cell constant of the cell?
The conductivity of 0.02 M KCl solution is 0.00250 ohm $^{-1} \mathrm{~cm}^{-1}$. What is its molar conductivity?
The molar conductivity of 0.01 M acetic acid at $25^{\circ} \mathrm{C}$ is $16.5 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ and its molar conductivity at zero concentration is $390.7 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$. What is its degree of dissociation?
Which of the following is released at cathode during electrolysis of aqueous sodium chloride?
Calculate the $\mathrm{E}_{\text {cell }}^{\circ}$ of $\mathrm{Al}\left|\mathrm{Al}_2\left(\mathrm{SO}_4\right)_{3(\mathrm{1M})}\right|\left|\mathrm{HCl}_{(\mathrm{IM})}\right| \mathrm{H}_{2(\mathrm{~g})(\mathrm{1atm})}, \mathrm{Pt}$ $\left(\right.$ Given $E_{\mathrm{AB}^{3+}|\mathrm{A}|}^0=-1.66 \mathrm{~V}$ )
Which of the following units of electrical measurement is not equivalent to 1 Siemen?
A conductivity cell dipped in 0.05 MKCl has resistance 600 ohm. If conductivity is $0.0012 \mathrm{ohm}^{-1} \mathrm{~cm}^{-1}$. What is the value of cell constant?
What is the conductivity of 0.05 M KCl solution if cell constant is $1.32 \mathrm{~cm}^{-1}$ and resistance is 528 ohm?
Which of the following substances conducts electricity?
Resistance and conductivity of a cell containing 0.1 M KCl solution at 298 K are 115 ohm and $1.90 \times 10^{-6} \mathrm{~S} \mathrm{~cm}^{-1}$ respectively. What is the value of cell constant?
Which of the following is used to avoid leakage of electrolyte in dry cell?
What is the quantity of electricity required to produce 4.8 g of Mg (molar mass $=24 \mathrm{~g} \mathrm{~mol}^{-1}$ ) from its salt solution?
For which electrolyte the molar conductivity at infinite dilution can not be obtained graphically?
What volume of chlorine gas (molar mass 71) is evolved at STP during electrolysis of fused NaCl by passage of 1 amp current for 965 second? (At STP, V $=22.4 \mathrm{~dm}^3$ )
If $\mathrm{E}^{\circ}$ cell for $\mathrm{Cd}_{(\mathrm{s})}\left|\mathrm{Cd}_{(\mathrm{IM})}^{2+} \square \mathrm{Ag}_{(1 \mathrm{M})}^{+}\right| \mathrm{Ag}_{(\mathrm{s})}$ is 1.2 V . What is the emf of the cell at $25^{\circ} \mathrm{C}$ ?
What is the conductivity of $0.02 \mathrm{~M} \mathrm{~AgNO}_3$ solution having cell constant $1.1 \mathrm{~cm}^{-1}$ and resistance is 94.5 ohms?
Which of the following expressions for conductivity of solution of an electrolyte is NOT correct?
Which of the following reactions occurs at cathode during discharging of lead accumulator?
The conductivity of 0.005 M NaI solution at $25^{\circ} \mathrm{C}$ is $6.07 \times 10^{-4} \Omega^{-1} \mathrm{~cm}^{-1}$. Calculate its molar conductivity
Calculate the amount of electricity required in coulombs to convert 0.08 mol of $\mathrm{MnO}_4^{-}$to $\mathrm{Mn}^{2+}$.
The limiting molar conductivities $\left(\Lambda_0\right)$ for NaCl , KBr and KCl are 126,152 and $150 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ respectively. What is the $\Lambda_0$ of NaBr ?
A conductivity cell dipped on 0.05 M KCl has resistance 600 ohm. If conductivity is $0.0015 \mathrm{ohm}^{-1} \mathrm{~cm}^{-1}$. What is the value of cell constant?
What is the cell constant, if two platinum electrodes in conductivity cell are separated by 0.92 cm and area of cross section is $1.2 \mathrm{~cm}^2$ ?
The molar conductivity of 0.02 M KCl solution is $410 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ at $25^{\circ} \mathrm{C}$. Calculate its conductivity?
Calculate the amount of electricity required to convert 1.1 mol of $\mathrm{Cr}_2 \mathrm{O}_7^{2-}$ to $\mathrm{Cr}^{+3}$ in acidic medium.
Which of the following statements is NOT correct for $\mathrm{H}_2-\mathrm{O}_2$ fuel cell?
The resistance of a conductivity cell of 0.1 M KCl solution is 120 ohm and conductivity is $1.64 \times 10^{-4} \mathrm{~S} \mathrm{~cm}^{-1}$. What is the value of cell constant?
Which of the following changes occurs during the discharging of lead accumulator?
Calculate the quantity of electricity required to liberate 0.1 mole of chlorine gas during electrolysis of molten sodium chloride.
Which from following expressions is used to calculate $\mathrm{E}_{\text {cell }}$ for the following cell at $25^{\circ} \mathrm{C}$ ?
$$\mathrm{Pb}_{(\mathrm{s})}\left|\mathrm{Pb}_{(\mathrm{1M})}^{++} \| \mathrm{Ag}_{(\mathrm{10M})}^{+}\right| \mathrm{Ag}_{(\mathrm{s})}$$
Which from following is NOT true about electrolysis of molten NaCl ?
The resistance of decimolar solution of NaCl is 30 ohms. Calculate the conductivity of solution if the cell constant is $0.33 \mathrm{~cm}^{-1}$.
A conductivity cell containing $$0.001 \mathrm{~M} \mathrm{~AgNO}_3$$ solution develops resistance $$6530 \mathrm{ohm}$$ at $$25^{\circ} \mathrm{C}$$. Calculate the electrical conductivity of solution at same temperature if the cell constant is $$0.653 \mathrm{~cm}^{-1}$$.
Calculate $$\mathrm{E}_{\text {cell }}^0$$ for $$\mathrm{Cd}_{(\mathrm{s})}\left|\mathrm{Cd}_{(\mathrm{1M})}^{++}\right|\left|\mathrm{Ag}_{(\mathrm{1M})}^{+}\right| \mathrm{Ag}_{(\mathrm{s})}$$.
$$\left[\mathrm{E}_{\mathrm{Cd}}^0=-0.403 \mathrm{~V} ; \mathrm{E}_{\mathrm{Ag}}^0=0.799 \mathrm{~V}\right.\text {]}$$
Which from following expressions is used to find the cell potential of $$\mathrm{Cd}_{(\mathrm{s})}\left|\mathrm{Cd}_{(\mathrm{aq})}^{++}\right|\left|\mathrm{Cu}_{(\mathrm{aq})}^{+}\right| \mathrm{Cu}_{(\mathrm{s})}$$ cell at $$25^{\circ} \mathrm{C}$$ ?
Which from following is NOT true about voltaic cell?
Calculate molar conductivity of $$\mathrm{NH}_4 \mathrm{OH}$$ at infinite dilution if molar conductivities of $$\mathrm{Ba}(\mathrm{OH})_2$$ $$\mathrm{BaCl}_2$$ and $$\mathrm{NH}_4 \mathrm{Cl}$$ at infinite dilution are $$520,280,129 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$$ respectively.
Which from the following expression represents molar conductivity of an electrolyte $$\mathrm{A}_2 B_3$$ type?
What is the molar conductivity of $$0.005 \mathrm{~M} \mathrm{~NaI}$$ solution if it's conductivity is $$6.065 \times 10^{-4} \Omega^{-1} \mathrm{~cm}^{-1} \text { ? }$$
Calculate $$E^{\circ}$$ cell for following.
$$\mathrm{Zn}(s)\left|\mathrm{Zn}^{++}(1 \mathrm{M}) \| \mathrm{Pb}^{++}(1 \mathrm{M})\right| \mathrm{Pb}(s)$$ if $$E_{\mathrm{Zn}}^{\circ}=-0.763 \mathrm{~V}$$ and $$E_{\mathrm{Pb}}^{\circ}=-0.126 \mathrm{~V}$$
Calculate $$\mathrm{E}_{\text {cell }}^0$$ if the equilibrium constant for following reaction is $$1.2 \times 10^6$$.
$$2 \mathrm{Cu}_{(\mathrm{aq})}^{+} \longrightarrow \mathrm{Cu}_{(\mathrm{aq})}^{++}+\mathrm{Cu}_{(\mathrm{s})}$$
Identify the overall oxidation reaction that occurs in lead storage cell during discharge.
Calculate the time required in second to deposit $$6.35 \mathrm{~g}$$ copper from its salt solution by passing 5 ampere current. [Molar mass of $$\mathrm{Cu}=63.5 \mathrm{~g} \mathrm{~mol}^{-1}$$ ]
Which of the following expressions represents molar conductivity of $$\mathrm{AB}_3$$ type electrolyte?
Calculate the $$\mathrm{E}_{\text {cell }}$$ for $$\mathrm{Zn}_{(\mathrm{s})}\left|\mathrm{Zn}_{(0.1 \mathrm{M})}^{++}\right|\left|\mathrm{Cr}_{(0.1 \mathrm{M})}^{+++}\right| \mathrm{Cr}_{(\mathrm{s})}$$ at $$25^{\circ} \mathrm{C}$$ if $$\mathrm{E}_{\text {cell }}^{\circ}$$ is $$0.02 \mathrm{~V}$$
A conductivity cell containing $$5 \times 10^{-4} \mathrm{~M} \mathrm{~NaCl}$$ solution develops resistance $$14000 \mathrm{~ohms}$$ at $$25^{\circ} \mathrm{C}$$. Calculate the conductivity of solution if the cell constant is $$0.84 \mathrm{~cm}^{-1}$$
Calculate $$\Delta \mathrm{G}^{\circ}$$ for the reaction $$\mathrm{Mg}_{(\mathrm{s})}+\mathrm{Sn}_{(\mathrm{aq})}^{++} \longrightarrow \mathrm{Mg}_{(\mathrm{aq})}^{++}+\mathrm{Sn}_{(\mathrm{s})}$$ if $$\mathrm{E}_{\text {cell }}^0$$ is $$2.23 \mathrm{~V}$$.
Electrolytic cells containing $$\mathrm{Zn}$$ and $$\mathrm{Al}$$ salt solutions are connected in series. If $$6.5 \mathrm{~g}$$ of $$\mathrm{Zn}$$ is deposited in one cell calculate mass of $$\mathrm{Al}$$ deposited in second cell (molar mass : $$\mathrm{Zn}=65, \mathrm{Al}=27$$ ) by passing definite quantity of electricity?
Which from following is strongest reducing agent?
Which from following sentences is NOT correct?
Calculate the $$\mathrm{E}_{\text {cell }}^{\circ}$$ for $$\mathrm{Zn}_{(\mathrm{s})}\left|\mathrm{Zn}_{(\mathrm{IM})}^{++}\right|\left|\mathrm{Cd}_{(\mathrm{IM})}^{++}\right| \mathrm{Cd}_{(\mathrm{s})}$$ at $$25^{\circ} \mathrm{C}\left[\mathrm{E}_{\mathrm{Zn}}^0=-0.763 \mathrm{~V} ; \mathrm{E}_{\mathrm{Cd}}^{\circ}=-0.403 \mathrm{~V}\right]$$
Find the number of faradays of electricity required to produce $$45 \mathrm{~g}$$ of $$\mathrm{Al}$$ from molten $$\mathrm{Al}_2 \mathrm{O}_3$$.
(At. mass of $$\mathrm{Al}=27$$ )
The molar conductivity of $$0.02 \mathrm{~M} \mathrm{~AgI}$$ at $$298 \mathrm{~K}$$ is $$142.3 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$$. What is its conductivity?
Which among the following is CORRECT formula for determination of cell constant?
What happens when solution of an electrolyte is diluted?
Calculate $$E_{\text {cell }}^{\circ}$$ in which following reaction occurs. $$\mathrm{Mg}_{(\mathrm{s})}+2 \mathrm{Ag}_{(\mathrm{IM})}^{+} \rightarrow \mathrm{Mg}_{(1 \mathrm{M})}^{+}+2 \mathrm{Ag}_{(\mathrm{s})}$$ if $$\mathrm{E}_{\mathrm{Ag}}^{\circ}=0.8 \mathrm{~V}$$ and $$\mathrm{E}_{\mathrm{Mg}}^{\circ}=-2.37 \mathrm{~V}$$
Calculate the conductivity of $$0.02 \mathrm{~M}$$ electrolyte solution if its molar conductivity $$407.2 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$$ ?
Conductivity of a solution is $$1.26 \times 10^{-2} \Omega^{-1} \mathrm{~cm}^{-1}$$ Calculate molar conductivity for $$0.01 \mathrm{~M}$$ solution.
Which of the following is NOT a difficulty in setting SHE?
What mass of $$\mathrm{Mg}$$ is produced during electrolysis of molten $$\mathrm{MgCl}_2$$ by passing $$2 \mathrm{~amp}$$ current for 482.5 second?
(Molar mass $$\mathrm{Mg}=24 \mathrm{~g} \mathrm{~mol}^{-1}$$)
What is the conductivity of $$0.05 ~\mathrm{M} ~\mathrm{BaCl}_2$$ solution if its molar conductivity is $$220 ~\Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$$ ?
A reaction, $$\mathrm{Ni}_{(\mathrm{s})}+\mathrm{Cu}_{(\mathrm{(M)})}^{+} \rightarrow \mathrm{Ni}_{(\mathrm{IM})}^{+}+\mathrm{Cu}_{(\mathrm{s})}$$ occurs in a cell. Calculate $$\mathrm{E}_{\text {cell }}^{\circ}$$ if $$\mathrm{E}_{\mathrm{Cu}}^{\circ}=0.337 \mathrm{~V}$$ and $$\mathrm{E}_{\mathrm{Ni}}^{\circ}=-0.257 \mathrm{~V}$$
Calculate $$\Delta \mathrm{G}^{\circ}$$ for the cell:
$$\mathrm{Sn}_{(\mathrm{s})}\left|\mathrm{Sn}_{(\mathrm{1M})}^{2+}\right|\left|\mathrm{Ag}_{(\mathrm{1M})}^{+}\right| \mathrm{Ag}_{(\mathrm{s})}$$ at $$25^{\circ} \mathrm{C}\left(\mathrm{E}_{\text {cell }}^{\circ}=0.90 \mathrm{~V}\right)$$
Calculate current in ampere required to deposit $$4.8 \mathrm{~g} ~\mathrm{Cu}$$ from it's salt solution in 30 minutes. [Molar mass of $$\mathrm{Cu}=63.5 \mathrm{~g} \mathrm{~mol}^{-1}$$ ]
Identify the gas produced due to reduction of $$\mathrm{NH}_4^{+}$$ ions at cathode during working of dry cell.
How long will it take to produce $$5.4 \mathrm{~g}$$ of $$\mathrm{Ag}$$ from molten $$\mathrm{AgCl}$$ by passing $$5 \mathrm{~amp}$$ current?
(Molar mass Ag = $$108 \mathrm{~g} \mathrm{~mol}^{-1}$$ )
Which of the following is NOT an example of secondary voltaic cell?
Calculate $$\wedge_0$$ of $$\mathrm{CH}_2 \mathrm{ClCOOH}$$ if $$\wedge_0$$ for $$\mathrm{HCl}, \mathrm{KCl}$$ and $$\mathrm{CH}_2 \mathrm{ClCOOK}$$ are $$4.2,1.5$$ and $$1.1 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$$ respectively?
The electrical conductance of unit volume (1 cm$$^3$$) of solution is called as
What is the conductivity of 0.02 M HCl solution if molar conductivity of the solution at 25$$^\circ$$C is 412.3 $$\Omega^{-1}$$ cm$$^{-1}$$ mol$$^{-1}$$ ?
What is the charge required for the reduction of moles of Cu$$^{2+}$$ to Cu?
The resistance of $$0.2 \mathrm{M}$$ solution of an electrolyte is 30 ohm and conductivity is $$1.2 \mathrm{~S} \mathrm{~m}^{-1}$$. What is the value of cell constant?
Which from the following is the correct relationship between standard Gibbs energy change and standard cell potential?
The conductivity of $$0.04 \mathrm{~M} \mathrm{~BaCl}_2$$ solution is $$0.0112 \Omega^{-1} \mathrm{~cm}^{-1}$$ at $$25^{\circ} \mathrm{C}$$. What is it's molar conductivity?
The conductivity of $$0.012 \mathrm{~M} \mathrm{~NaBr}$$ solution is $$2.67 \times 10^{-4} \mathrm{~S} \mathrm{~cm}^{-1}$$. What is it's molar conductivity?
During the electrolysis of fused $$\mathrm{NaCl}$$, the product obtained at anode is
What is the weight of $$\mathrm{Al}$$ deposited at cathode when 1 ampere current is passed through molten $$\mathrm{AlCl}_3$$ for 9650 seconds? (At mass of $$\mathrm{Al}=27$$)
How many electrons flow through the wire if a current of 1.5 ampere flow through it for 3 hours?
The conductivity of $$0.3 \mathrm{M}$$ solution of $$\mathrm{KCl}$$ at $$298 \mathrm{~K}$$ is $$0.0627 \mathrm{~S} \mathrm{~cm}^{-1}$$. What is it's molar conductivity?
In the cell represented as $$\mathrm{Ni}_{(\mathrm{s})}\left|\mathrm{Ni}_{(\mathrm{IM})}^{2 \oplus}\right|\left|\mathrm{Ag}_{(\mathrm{IM})}^{\oplus}\right| \mathrm{Ag}_{(\mathrm{s})}$$, the reducing agent is
How many Faraday of electricity is required to deposit $$0.8 \mathrm{~g}$$ of calcium at cathode by the electrolysis of $$\mathrm{CaCl}_2$$ ?
(Molar mass of $$\mathrm{Ca}=40 \mathrm{~g} \mathrm{~mol}^{-1}$$)
What is the conductivity of $$0.02 \mathrm{~M} \mathrm{~KCl}$$ solution if cell constant is $$1.29 \mathrm{~cm}^{-1}$$ with resistance 645 $$\Omega$$ ?
Electrical conductance due to all the ions in $$1 \mathrm{~cm}^3$$ of given solution is called as
What is the resistance of $$0.01 ~\mathrm{M} ~\mathrm{KCl}$$ solution if its conductivity is $$200 ~\mathrm{ohm}^{-1} \mathrm{cn}^{-1}$$ and cell constant is $$1 \mathrm{~cm}^{-1}$$ ?
Molar conductivity of 0.04 M BaCl$$_2$$ solution is 230 $$\Omega^{-1}$$ cm$$^2$$ mol$$^{-1}$$ at 27$$^\circ$$C. What is it's conductivity?
Which from following electrolytes, molar conductivity is determined using Kohlrausch theory?
Which among the following statements is true for Galvanic cell?
What will be the concentration of solution of electrolyte if it's molar conductivity and conductivity are respectively 230 $$\Omega^{-1}$$ cm$$^2$$ mol$$^{-1}$$ and 0.0115 $$\Omega^{-1}$$ cm$$^{-1}$$ at 298 K?
What is the number of moles of electrons passed when current of 5 ampere is passed through a solution of FeCl$$_3$$ for 20 minutes?
Which among the following statements is true for conductivity?
The molar conductivity of $$0.4 \mathrm{~M} \mathrm{~KCl}$$ solution is $$2.5 \times 10^5 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$$. What is the resistivity of solution?
What is the number of electrons passed through an electrolyte solution when 1 ampere current is passed for 16.1 minutes?
Which among the following aqueous salt solution is used in conductivity cell to determine cell constant?
What is the molar conductivity of $$0.05 \mathrm{M}$$ solution of sodium hydroxide, if it's conductivity is $$0.0118 \mathrm{~S} \mathrm{~cm}^{-1}$$ at $$298 \mathrm{~K}$$ ?
How many faraday of electricity is required to produce 10 g of calcium metal (molar mass = 40 g mol$$^{-1}$$) from calcium ions?
The molar conductivity of 0.1 M BaCl$$_2$$ solution is 106 $$\Omega^{-1}$$ cm$$^2$$ mol$$^{-1}$$ at 25$$^\circ$$C. What is it's conductivity?
Which from following is NOT correct regarding electrolysis?
A conductivity cell shows resistance of 600 ohm. If conductivity of 0.01 M KCl is 0.0015 $$\Omega^{-1}$$ cm$$^{-1}$$, what is cell constant?
How many Faradays of electricity is required to produce 4.8 g of Mg at cathode in the electrolysis of molten $\mathrm{MgCl}_2$ ? (Molar mass of $\mathrm{Mg}=24 \mathrm{~g} / \mathrm{mol}$ )
What is the SI unit for electrochemical equivalent?
Number of electrons involved in the reaction, when 1 Faraday of electricity is passed through an electrolytic solution is
A solution of $$\mathrm{CuSO}_4$$ is electrolysed using a current of 1.5 amperes for 10 minutes. What mass of Cu is deposited at cathode? [Atomic mass of $$\mathrm{Cu}=63.7$$]
If resistivity of 0.8 M KCl solution is $$2.5 \times 10^{-3} \Omega \mathrm{~cm}$$. Calculate molar conductivity solution?
How many electrons are involved in the reaction, when $$0.40 \mathrm{~F}$$ of electricity is passed through an electrolytic solution?
What will be the concentration of $$\mathrm{NaCl}$$ solution, if the molar conductivity and conductivity of $$\mathrm{NaCl}$$ solution is $$124.3 \Omega^{-1} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$$ and $$1.243 \times 10^{-4} \Omega^{-1} \mathrm{~cm}^2$$ respectively?
Which among the following is correct for electrolysis of brine solution?
In the electrolysis of aqueous sodium chloride with inert electrodes the products obtained at anode and cathode respectively are
Calculate E.M.F. of following cell at 298 K $\mathrm{Zn}(s)\left|\mathrm{ZnSO}_4(0.01 \mathrm{M})\right|\left|\mathrm{CuSO}_4(1.0 \mathrm{M})\right| \mathrm{Cu}(\mathrm{s})$ if $\mathrm{E}^{\circ}$ cell $=2.0 \mathrm{~V}$
The SI unit of electrochemical equivalent is
The molar conductivities at infinite dilution for sodium acetate, HCl and NaCl are $91 \mathrm{~S} \mathrm{~cm}{ }^2$ $\mathrm{mol}^{-1}, 425.9 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$ and $12.6 .4 \mathrm{~S} \mathrm{~cm}^2$ $\mathrm{mol}^{-1}$ respectively. The molar conductivity of acetic acid at infinite dilution is
Which of the following acts as oxidising agent in hydrogen-oxygen fuel cell ?
Standard hydrogen electrode (SHE) is a
The conductivity of an electrolytic solution decreases on dilution due to
Two electrolytic cells are connected in series containing $\mathrm{CuSO}_4$ solution and molten $\mathrm{AlCl}_3$. If in electrolysis 0.4 moles of 'Cu' are deposited on cathode of first cell. The number of moles of 'Al' deposited on cathode of the second cell is
The resistance of $\frac{1}{10} M$ solution is $25 \times 10^3$ ohm. What is the molar conductivity of solution? (cell constant $=1.25 \mathrm{~cm}^{-1}$)