JEE Main 2015 (Offline) | Thermodynamics Question 150 | Chemistry

The following reaction is performed at 298 K
2NO(g) + O₂ (g) $$\leftrightharpoons$$ 2NO₂ (g)
The standard free energy of formation of NO(g) is 86.6 kJ/mol at 298 K. What is the standard free energy of formation of NO₂(g) at 298 K? (KP = 1.6 × 10¹²)

86600 + R(298) ln(1.6 $$\times$$ 10¹²)

86600 - $$ln (1.6 \times 10^{12}) \over R (298)$$

0.5[2×86,600 – R(298) ln(1.6×10¹²)]

R(298) ln(1.6×10¹²) – 86600

JEE Main 2014 (Offline)

MCQ (Single Correct Answer)

-1

For complete combustion of ethanol, C₂H₅OH(l) + 3O₂(g) $$\to$$ 2CO₂(g) + 3H₂O(l) the amount of heat produced as measured in bomb calorimeter, is 1364.47 kJ mol^–1 at 25^oC. Assuming ideality the Enthalpy of combustion, $$\Delta _CH$$, for the reaction will be : (R = 8.314 kJ mol^–1)

–1460.50 kJ mol^–1

– 1350.50 kJ mol^–1

– 1366.95 kJ mol^–1

– 1361.95 kJ mol^–1

JEE Main 2013 (Offline)

MCQ (Single Correct Answer)

-1

A piston filled with 0.04 mol of an ideal gas expands reversibly from 50.0 mL to 375 mL at a constant temperature of 37.0^oC. As it does so, it absorbs 208J of heat. The values of q and w for the process will be :
(R = 8.314 J/mol K) ( l n 7.5 = 2.01)

q = – 208 J, w = – 208 J

q = – 208 J, w = + 208 J

q = + 208 J, w = + 208 J

q = + 208 J, w = – 208 J

AIEEE 2012

MCQ (Single Correct Answer)

-1

The incorrect expression among the following is :

$${{\Delta {G_{system}}} \over {\Delta {S_{total}}}} = - T$$

In isothermal process $${w_{reversible}}$$ = $$ - nRT\,\ln \,{{{V_f}} \over {{V_i}}}$$

In $$K\, = {{\Delta {H^o} - T\Delta {S^o}} \over {RT}}$$

$$K\, = \,{e^{ - \Delta {G^o}/RT}}$$