1
JEE Main 2014 (Offline)
+4
-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 25oC. Assuming ideality the Enthalpy of combustion, $$\Delta _CH$$, for the reaction will be : (R = 8.314 kJ mol–1)
A
–1460.50 kJ mol–1
B
– 1350.50 kJ mol–1
C
– 1366.95 kJ mol–1
D
– 1361.95 kJ mol–1
2
JEE Main 2013 (Offline)
+4
-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 37.0oC. 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)
A
q = – 208 J, w = – 208 J
B
q = – 208 J, w = + 208 J
C
q = + 208 J, w = + 208 J
D
q = + 208 J, w = – 208 J
3
AIEEE 2012
+4
-1
The incorrect expression among the following is :
A
$${{\Delta {G_{system}}} \over {\Delta {S_{total}}}} = - T$$
B
In isothermal process $${w_{reversible}}$$ = $$- nRT\,\ln \,{{{V_f}} \over {{V_i}}}$$
C
In $$K\, = {{\Delta {H^o} - T\Delta {S^o}} \over {RT}}$$
D
$$K\, = \,{e^{ - \Delta {G^o}/RT}}$$
4
AIEEE 2011
+4
-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 27oC is :
A
35.8 J mol-1 K−1
B
32.3 J mol-1 K−1
C
42.3 J mol-1 K−1
D
38.3 J mol-1 K−1
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