# Thermodynamics Exam For 12th Grade! Quiz

30 Questions | Total Attempts: 66  Settings  .

• 1.
A well stoppered Thermo flask containing some ice cubes is an example of
• A.

Closed system

• B.

Open system

• C.

Isolated system

• D.

Non thermodynamic system

• 2.
Identify the intensive quantity from the following.
• A.

Enthalpy and temperature

• B.

Volume and temperature

• C.

Enthalpy and volume

• D.

Temperature and refractive index

• 3.
For an adiabatic process, which of the following is correct?
• A.

Q = 0

• B.

P∆V = 0

• C.

∆E = 0

• D.

Q = + W

• 4.
In which of the following, work behaves as a state function?
• A.

Isothermal

• B.

• C.

Isobaric

• D.

Isochoric

• 5.
When a gas is compressed adiabatically and reversibly the final temperature is:
• A.

Higher than the initial temperature

• B.

Lower than the initial temperature

• C.

The same as initial temperature

• D.

Dependent upon the rate of compression

• 6.
Q = -w is not true for
• A.

Isothermal

• B.

• C.

Cyclic process

• D.

Both 1 & 3

• 7.
The temperature of an ideal gas increases in an:
• A.

• B.

Isothermal expansion

• C.

• D.

Isothermal compression

• 8.
Which one is a state function:-
• A.

Heat supplied at constant pressure

• B.

Heat supplied at constant volume

• C.

Enthalpy

• D.

All of the above

• 9.
The work is done by a weightless piston in causing an expansion ΔV (at constant temperature), when the opposing pressure P is variable. What will be the final expression of the work?
• A.

W = - ∫ P∆V

• B.

W= - PΔV

• C.

W = 0

• D.

None of these

• 10.
The work done by 100 calorie of heat in isothermal expansion of ideal gas is:
• A.

418.4 J

• B.

4.184 J

• C.

41.84 J

• D.

None

• 11.
Temperature and heat are not:
• A.

Extensive properties

• B.

Intensive properties

• C.

Intensive and extensive properties respectively

• D.

Extensive and intensive properties respectively

• 12.
One mole of gas absorbs 200 J of heat at constant volume. Its temperature rises from 298 K to 308 K. The change in internal energy is:
• A.

-200 J

• B.

400 J

• C.

200 J

• D.

- 400 j

• 13.
Which statement is true for the reversible process:-
• A.

It takes place in single step

• B.

Driving force is much greater than opposing force

• C.

Work obtain is minimum

• D.

None

• 14.
Both q & w are __________ function & q + w is a ___________ function.
• A.

State, State

• B.

State, path

• C.

Path, state

• D.

Path, path

• 15.
The work done by a system is 8J when 40 J  heat is supplied to it. Calculate the increases in internal energy of the system.
• A.

32 J

• B.

42 J

• C.

48 J

• D.

- 32 J

• 16.
Under which of the following conditions is the relation ΔH=ΔE+PΔV valid for a closed system?
• A.

Constant pressure

• B.

Constant temperature

• C.

Constant temperature and pressure

• D.

Constant temperature pressure and composition

• 17.
ΔvapH for water at 100°C is 40.66 kJ mol-1  The internal energy of vaporization of water at 100°C (in KJ)
• A.

37.53

• B.

39.08

• C.

42.19

• D.

43.73

• 18.
The difference between heats of reaction at constant pressure and constant volume for the reaction, 2C6H6 (l)+15 O2 (g) → 12CO2(g)+ 6H2O(l) at 25°C in kJ is:
• A.

7.43

• B.

-7.43

• C.

3.72

• D.

-3.72

• 19.
For a gaseous reaction, A(g) + 3B(g) → 3C(g) + 3D(g) ∆E is 17 kCal at 27°C assuming R = 2 Cal /Kmol, the value of ∆H for the above reaction is:
• A.

15.8 Kcal

• B.

18.2 Kcal

• C.

20.0 Kcal

• D.

16.4 Kcal

• 20.
For CaCO3​(s)→CaO(s)+CO2​(g ) at 977°C, ΔH=174 kJ/mol; then ΔE is:
• A.

160 KJ

• B.

163.6 KJ

• C.

186.4 KJ

• D.

180 KJ

• 21.
The difference in ΔH and ΔU for combustion of methane for the combustion of methane at 250C would be:
• A.

Zero

• B.

2 x 298 x -2 cals

• C.

2 x 298 x -3 cals

• D.

2 x 25 x -3 cals

• 22.
For the system S(s) + O2(g) → SO2(g)
• A.

ΔH = ΔE

• B.

ΔH > ΔE

• C.

ΔE > ΔH

• D.

ΔH = 0

• 23.
ΔS for the reaction :  MgCO3(s) → MgO(s) + CO2(g) will be:
• A.

0

• B.

-ve

• C.

+ve

• D.

Infinity

• 24.
In which of the following cases, entropy will decrease:
• A.

Solid changing to liquid

• B.

Expansion of gas

• C.

Crystal dissolve

• D.

Polymerization

• 25.
For the reaction Ag2O(s) → 2Ag(s) + 1/2 O2(g), the value of ΔH=30.56 KJ/mol and ΔS=66 J/Kmol. The temperature at which the free energy change for the reaction will be zero is:
• A.

373 K

• B.

413 K

• C.

463 K

• D.

493 K

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