Chapter 5: Thermodynamics MCQs | chemistry Class 11 CBSE

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Question 1

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A thermodynamic state function is a quantity

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Question 2

Objective

In an open system, which of the following exchanges can occur with the surroundings?

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Question 3

Objective

For an adiabatic process, the correct condition is:

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Question 4

Objective

The enthalpies of all elements in their standard states are:

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Question 5

Objective

For a reaction in which ΔU° of combustion of methane is -X kJ mol-1, the value of ΔH° compared to ΔU° for CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) is:

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Question 6

Objective

The enthalpy of combustion of methane, graphite and dihydrogen at 298 K are -890.3 kJ mol-1, -393.5 kJ mol-1 and -285.8 kJ mol-1 respectively. The enthalpy of formation of CH4(g) is:

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Question 7

Objective

A reaction A + B → C + D + q has a positive entropy change. The reaction will be:

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Question 8

Objective

Which of the following correctly represents the first law of thermodynamics?

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Question 9

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For free expansion of an ideal gas in vacuum, which of the following is correct?

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Question 10

Objective

Enthalpy H is defined as:

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Question 11

Objective

The relationship between Cp and CV for an ideal gas is:

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Question 12

Objective

In a bomb calorimeter, the reaction is carried out at:

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Question 13

Objective

For the reaction N2(g) + 3H2(g) → 2NH3(g), the value of Δng is:

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Question 14

Objective

The standard state of a substance at a specified temperature is:

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Question 15

Objective

Which of the following phase changes involves a positive enthalpy change (endothermic)?

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Question 16

Objective

For reversible isothermal expansion of n mol of ideal gas from Vi to Vf, the work done on the gas is:

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Question 17

Objective

Hess's law is based on the fact that enthalpy is a:

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Question 18

Objective

When a thermochemical equation is reversed, the value of ΔrH is:

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Question 19

Objective

The mean C-H bond enthalpy in methane, given ΔaH°(CH4) = 1665 kJ mol-1, is:

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Question 20

Objective

Lattice enthalpy of NaCl cannot be measured directly because:

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Chapter 5: Thermodynamics | MCQs

A thermodynamic state function is a quantity

In an open system, which of the following exchanges can occur with the surroundings?

For an adiabatic process, the correct condition is:

The enthalpies of all elements in their standard states are:

For a reaction in which ΔU° of combustion of methane is -X kJ mol-1, the value of ΔH° compared to ΔU° for CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) is:

The enthalpy of combustion of methane, graphite and dihydrogen at 298 K are -890.3 kJ mol-1, -393.5 kJ mol-1 and -285.8 kJ mol-1 respectively. The enthalpy of formation of CH4(g) is:

A reaction A + B → C + D + q has a positive entropy change. The reaction will be:

Which of the following correctly represents the first law of thermodynamics?

For free expansion of an ideal gas in vacuum, which of the following is correct?

Enthalpy H is defined as:

The relationship between Cp and CV for an ideal gas is:

In a bomb calorimeter, the reaction is carried out at:

For the reaction N2(g) + 3H2(g) → 2NH3(g), the value of Δng is:

The standard state of a substance at a specified temperature is:

Which of the following phase changes involves a positive enthalpy change (endothermic)?

For reversible isothermal expansion of n mol of ideal gas from Vi to Vf, the work done on the gas is:

Hess's law is based on the fact that enthalpy is a:

When a thermochemical equation is reversed, the value of ΔrH is:

The mean C-H bond enthalpy in methane, given ΔaH°(CH4) = 1665 kJ mol-1, is:

Lattice enthalpy of NaCl cannot be measured directly because:

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