Topic: Thermodynamics, Test No.: 01, Total MCQs: 15
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Question 1 |
Standard enthalpy of vapourisation DvapHQ for water at 100° C is 40.66 kJmol–1. The internal energy of vapourisation of water at 100°C (in kJmol–1) is
(Assume water vapour to behave like an ideal gas) [CBSE AIPMT 2012]
+43.76 | |
+40.66 | |
+37.56 | |
–43.76 |
Question 2 |
The enthalpy of fusion of water is 1.435 kcal/mol. The molar entropy change for the melting of ice at 0°C is [CBSE AIPMT 2012]
5.260 cal/(mol K) | |
0.526 cal/(mol K) | |
10.52 cal/(mol K) | |
21.04 cal/(mol K) |
Question 3 |
Consider the reaction :
4NO2(g) + O2(g) ® 2N2O5(g), ΔrH = –111kJ.
If N2O5(s) is formed instead of N2O5(g) in the above reaction, the ΔrH value will be:
(given, ΔH of sublimation for N2O5 is 54 kJ mol–1) [AIEEE 2011]
–219 kJ | |
–165 kJ | |
+ 54 kJ | |
+ 219 kJ |
Question 4 |
Based on the first law of thermodynamics, which one of the following is correct? [Karnataka CET 2011]
For an isothermal process, q = +w | |
For an isochoric process, ΔU = -q | |
For an adiabatic process, ΔU = -w | |
For a cyclic process, q = -w |
Question 5 |
The amount of the heat released when 20 ml 0.5 M NaOH is mixed with 100 ml 0.1 M HCl is x kJ. The heat of neutralization is [West Bengal JEE 2011]
– 100 x kJ/mol | |
– 50 x kJ/mol | |
+ 100 x kJ/mol | |
+50 x kJ/mol |
Question 6 |
The bond energy (in kcal mol–1) of a C—C single bond is approximately [IIT JEE 2010]
1 | |
10 | |
100 | |
1000 |
Question 7 |
The species which by definition has ZERO standard molar enthalpy of formation at 298 K is [IIT JEE 2010]
Br2(g) | |
Cl2(g) | |
H2O(g) | |
CH4(g) |
Question 8 |
The standard enthalpy of formation of NH3 is –46.0 kJ mol–1. If the enthalpy of formation of H2 from its atoms is –436 kJ mol–1 and that of N2 is –712 kJ mol–1, the average bond enthalpy of N — H bond is NH3 is [AIEEE 2010]
–1102 kJ mol–1 | |
–964 kJ mol–1 | |
+352 kJ mol–1 | |
+1056 kJ mol–1 |
Question 9 |
The amount of heat evolved when 500 cm3 of 0.1 M HCl is mixed with 200 cm3 of 0.2 M NaOH is ______. [Karnataka CET 2010]
1.292 kJ | |
2.292 kJ | |
3.392 kJ | |
0.292 kJ |
Question 10 |
In a constant volume calorimeter, 3.5 g of a gas with molecular weight 28 was burnt in excess oxygen at 298.0 K. The temperature of the calorimeter was found to increase from 298.0 K to 298.45 K due to the combustion process. Given that the heat capacity of the calorimeter is 2.5 kJ K−1, the numerical value for the enthalpy of combustion of the gas in kJ mol−1 is [IIT JEE 2009]
3 | |
7 | |
8 | |
9 |
Question 11 |
If one mole of ammonia and one mole of hydrogen chloride are mixed in a closed container to form ammonium chloride gas, then [Karnataka CET 2008]
ΔH > Δu | |
ΔH = Δu | |
ΔH < Δu | |
there is no relationship |
Question 12 |
Which of the following is an intensive property? [Karnataka CET 2007]
temperature | |
surface tension | |
viscosity | |
all of these |
Question 13 |
An ideal gas is allowed to expand both reversibly and irreversibly in an isolated system. If Ti is the initial temperature and Tf is the final temperature, which of the following statements is correct? [AIEEE 2006]
(Tf)irrev > (Tf)rev | |
Tf > Ti for reversible process but Tf = Ti for irreversible process | |
(Tf)rev = (Tf)irrev | |
Tf = Ti for both reversible and irreversible processes |
Question 14 |
The standard enthalpy of formation (ΔfH°) at 298 K for methane, CH4(g), is –74.8 kJ mol–1. The additional information required to determine the average energy for C – H bond formation would be [AIEEE 2006]
the dissociation energy of H2 and enthalpy of sublimation of carbon | |
latent heat of vaporization of methane | |
the first four ionization energies of carbon and electron gain enthalpy of hydrogen | |
the dissociation energy of hydrogen molecule, H2 |
Question 15 |
The temperature of the system .decreases in an ______. [Karnataka CET 2005]
adiabatic compression | |
isothermal expansion | |
isothermal compression | |
adiabatic expansion |