JEE Main 2014 (Offline) | Thermodynamics Question 150 | Chemistry

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

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

AIEEE 2011

MCQ (Single Correct Answer)

-1

The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of 10 dm³ to a volume of 100 dm³ at 27^oC is :

35.8 J mol^-1 K⁻¹

32.3 J mol^-1 K⁻¹

42.3 J mol^-1 K⁻¹

38.3 J mol^-1 K⁻¹

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