Thermodynamics - 1

Question 1

The pressure-volume work for an ideal gas can be calculated using the expression

This type of work can also be calculated using the area under the curve within the specified limits. When an ideal gas is compressed, (I) reversibly or (II) irreversibly, then

Accepted Answer

W(I) > W(II)

Answer

W(I) = W(II)

Answer

W(I) < W(II)

Answer

W(I) = W(II) + p_exΔV

Question 2

In the following case, find the option with the correct matching

Accepted Answer

a

Answer

b

Answer

c

Answer

d

Question 3

1.0 mole of a monoatomic ideal gas is expanded from state I to state II at 300 K.

Thus, work done is

Accepted Answer

-1729 J

Answer

+1729 J

Answer

-75.8 J

Answer

17.07 J

Question 4

1 mole of a diatomic gas is contained in a piston. It gains 50.0 J of heat and work is done on the surrounding by the system is -100 J. Thus,

Accepted Answer

the gas will cool by 2.41°

Answer

he gas will heat by 2.41°

Answer

the gas will cool by 3.61°

Answer

he gas will heat by 3.61°

Question 5

A sample containing 1.0 mole of an ideal gas is expanded isothermally and reversibly to ten time of its original volume, in two separate experiments. The expansion is carried out 300 K and at 600 K, respectively. Choose the correct option.

Accepted Answer

Question 6

Change in enthalpy for reaction,
2H₂O_2(l) → 2H₂O_(l) + O_2(g)
if heat of formation of H₂O_2(l)and H₂O_(l)are −188 and −286 kJ/mol respectively, is

Accepted Answer

–196 kJ/mol

Answer

+196 kJ/mol

Answer

+948 kJ/mol

Answer

–948 kJ/mol

Question 7

If ΔH is the change in enthalpy and ΔE, the change in internal energy accompanying a gaseous reaction, then

Accepted Answer

ΔH < ΔE only if the number of moles of products is less than the number of moles of the reactants.

Answer

ΔH is always greater than ΔE

Answer

ΔH < ΔE only if the number of moles of the products is greater than the number of moles of the reactants

Answer

ΔH is always less than ΔE

Question 8

During compression of a spring the work done is 10 kJ and 2 kJ escaped to the surroundings as heat. The change in internal energy, ΔU (in kJ) is :

Accepted Answer

8

Answer

12

Answer

&ndash;8

Answer

&ndash;12

Question 9

Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The enthalpy change (in kJ) for the process is

Accepted Answer

0 kJ

Answer

11.4 kJ

Answer

&ndash;11.4 kJ

Answer

4.8 kJ

Question 10

When 5 litres of a gas mixture of methane and propane is perfectly combusted at 0°C and 1 atmosphere, 16 litres of oxygen at the same temperature and pressure is consumed. The amount of heat released from this combustion in kJ (ΔH_comb. (CH₄) = 890 kJ mol⁻¹, ΔH_comb. (C₃H₈) = 2220 kJ mol⁻¹) is

Accepted Answer

317

Answer

38

Answer

477

Answer

32

Question 11

Consider the following reactions:

Enthalpy of formaton of H₂O(l)

Accepted Answer

-X₂ kJ mol⁻¹

Answer

+X₃ kJ mol⁻¹

Answer

-X₄ kJ mol⁻¹

Answer

+X₁ kJ mol⁻¹

Question 12

The correct relationship between free energy change in a reaction and the corresponding equilibrium constant
K_c is

Accepted Answer

-ΔG° = RT ln K_c

Answer

-ΔG = RT ln K_c

Answer

ΔG° = RT ln K_c

Answer

ΔG = RT ln K_c

Question 13

Accepted Answer

Answer

Answer

Answer

Question 14

Accepted Answer

1110 K

Answer

910 K

Answer

510 K

Answer

710 K

Question 15

Accepted Answer

Answer

Answer

Answer

Question 16

Accepted Answer

–3RT

Answer

+RT

Answer

+3RT

Answer

–RT

Question 17

Accepted Answer

5.260 cal/(mol K)

Answer

10.52 cal/(mol K)

Answer

21.04 cal/(mol K)

Answer

0.526 cal/(mol K)

Question 18

Accepted Answer

Cl2 (g)

Answer

Br2 (g)

Answer

H2O (g)

Answer

CH4 (g)

Question 19

Accepted Answer

positive

Answer

negative

Answer

zero

Answer

constant

Question 20

Accepted Answer

Answer

Answer

Answer

Question 21

Accepted Answer

Answer

Answer

Answer

Question 22

Accepted Answer

–17 kcal

Answer

–111 kcal

Answer

–170 kcal

Answer

–85 kcal

Question 23

For silver, C_p(JK^–1 mol^–1) = 23 + 0.01 T. If the temperature (T) of 3 moles of silver is raised from 300 K to 1000 K at 1 atm pressure, the value of ΔH will be close to -

Accepted Answer

62 kJ

Answer

13 kJ

Answer

16 kJ

Answer

21 kJ

Question 24

Accepted Answer

Answer

Answer

Answer

Question 25

Accepted Answer

-175 kJ/mol

Answer

525 kJ/mol

Answer

-325 kJ/mol

Answer

325 kJ/mol

Question 26

Accepted Answer

Answer

Answer

Answer

Question 27

Accepted Answer

373.4 K

Answer

273.4 K

Answer

393.4 K

Answer

293.4 K

Question 28

Accepted Answer

Answer

Answer

Answer

Question 29

Accepted Answer

1118 K

Answer

1008 K

Answer

1200 K

Answer

845 K

Question 30

Accepted Answer

9.2

Answer

92.1

Answer

0

Answer

4

Thermodynamics - 1 - Free MCQ Test with solutions for JEE Chemistry

MCQ Practice Test & Solutions: Thermodynamics - 1 (30 Questions)

The pressure-volume work for an ideal gas can be calculated using the expression
This type of work can also be calculated using the area under the curve within the specified limits. When an ideal gas is compressed, (I) reversibly or (II) irreversibly, then

In the following case, find the option with the correct matching

1.0 mole of a monoatomic ideal gas is expanded from state I to state II at 300 K.
Thus, work done is

1 mole of a diatomic gas is contained in a piston. It gains 50.0 J of heat and work is done on the surrounding by the system is -100 J. Thus,

A sample containing 1.0 mole of an ideal gas is expanded isothermally and reversibly to ten time of its original volume, in two separate experiments. The expansion is carried out 300 K and at 600 K, respectively. Choose the correct option.

Change in enthalpy for reaction,
2H₂O_2(l) → 2H₂O_(l) + O_2(g)
if heat of formation of H₂O_2(l)and H₂O_(l)are −188 and −286 kJ/mol respectively, is

If ΔH is the change in enthalpy and ΔE, the change in internal energy accompanying a gaseous reaction, then

During compression of a spring the work done is 10 kJ and 2 kJ escaped to the surroundings as heat. The change in internal energy, ΔU (in kJ) is :

Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The enthalpy change (in kJ) for the process is

Consider the following reactions:
Enthalpy of formaton of H₂O(l)

The correct relationship between free energy change in a reaction and the corresponding equilibrium constant
K_c is

For silver, C_p(JK^–1 mol^–1) = 23 + 0.01 T. If the temperature (T) of 3 moles of silver is raised from 300 K to 1000 K at 1 atm pressure, the value of ΔH will be close to -

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Thermodynamics - 1 - Free MCQ Test with solutions for JEE Chemistry

MCQ Practice Test & Solutions: Thermodynamics - 1 (30 Questions)

The pressure-volume work for an ideal gas can be calculated using the expressionThis type of work can also be calculated using the area under the curve within the specified limits. When an ideal gas is compressed, (I) reversibly or (II) irreversibly, then

In the following case, find the option with the correct matching

1.0 mole of a monoatomic ideal gas is expanded from state I to state II at 300 K.Thus, work done is

1 mole of a diatomic gas is contained in a piston. It gains 50.0 J of heat and work is done on the surrounding by the system is -100 J. Thus,

A sample containing 1.0 mole of an ideal gas is expanded isothermally and reversibly to ten time of its original volume, in two separate experiments. The expansion is carried out 300 K and at 600 K, respectively. Choose the correct option.

Change in enthalpy for reaction, 2H2O2(l) → 2H2O(l) + O2(g) if heat of formation of H2O2(l) and H2O(l) are −188 and −286 kJ/mol respectively, is

If ΔH is the change in enthalpy and ΔE, the change in internal energy accompanying a gaseous reaction, then

During compression of a spring the work done is 10 kJ and 2 kJ escaped to the surroundings as heat. The change in internal energy, ΔU (in kJ) is :

Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The enthalpy change (in kJ) for the process is

Consider the following reactions:Enthalpy of formaton of H2O(l)

The correct relationship between free energy change in a reaction and the corresponding equilibrium constant Kc is

For silver, Cp(JK–1 mol–1) = 23 + 0.01 T. If the temperature (T) of 3 moles of silver is raised from 300 K to 1000 K at 1 atm pressure, the value of ΔH will be close to -

Chemistry for JEE Main & Advanced

Chemistry for JEE Main & Advanced

Top Courses for JEE

About this JEE Practice Test

Explore more JEE Study Resources

The pressure-volume work for an ideal gas can be calculated using the expression
This type of work can also be calculated using the area under the curve within the specified limits. When an ideal gas is compressed, (I) reversibly or (II) irreversibly, then

1.0 mole of a monoatomic ideal gas is expanded from state I to state II at 300 K.
Thus, work done is

Change in enthalpy for reaction,
2H₂O_2(l) → 2H₂O_(l) + O_2(g)
if heat of formation of H₂O_2(l)and H₂O_(l)are −188 and −286 kJ/mol respectively, is

Consider the following reactions:
Enthalpy of formaton of H₂O(l)

The correct relationship between free energy change in a reaction and the corresponding equilibrium constant
K_c is

For silver, C_p(JK^–1 mol^–1) = 23 + 0.01 T. If the temperature (T) of 3 moles of silver is raised from 300 K to 1000 K at 1 atm pressure, the value of ΔH will be close to -