STANDARD Chemistry Thermodynamics Class 11 Questions

System in which there is no exchange of matter, work or energy from surroundings is

U = q + w, is mathematical expression for

The work done during the expansion of a gas from 4 dm³ to 6 dm³ against a constant external pressure of 3 atm is (1 L atm = 101.32 J)

If w is the amount of work done by the system and q is the amount of heat supplied to the system, identify the type system of the system.

A process is called reversible when

For an isothermal reversible expansion process, the value of q can be calculated by the expression

In an adiabatic expansion of ideal gas

Two litres of an ideal gas at a pressure of 10 atm expands isothermally into a vacuum until its total volume is 10 litres. How much heat is absorbed and how much work is done in the expansion?

The enthalpy change of a reaction does not depend upon

Consider the given diagram for 1 mole of a gas X and answer the following question. The process A → B represents

Which of the following relationships is not correct for the relation between ΔH and ΔU?

According to the first law of thermodynamics, ΔU = q + w. In special cases the statement can be expressed in different ways. Which of the following is not a correct expression?

A system changes from state X to Y with a change in internal energy measuring to 25 kJ mol⁻¹, by a reversible path and returns from Y to X by an irreversible path. What will be the net change in internal energy?

200 joules of heat was supplied to a system at constant volume. It resulted in the increase in temperature of the system from 29R to 323 K. What is the change in internal energy of the system?

In thermodynamics, which one of the following properties is not an intensive property?

The molar heat capacity of water at constant pressure, Cₚ is 75 J K⁻¹ mol⁻¹. When 10 kJ of heat is supplied to 1 kg water which is free to expand, the increase in temperature of water is

For the reaction of one mole of zinc dust with one mole of sulphuric acid in a bomb calorimeter, ΔU and w correspond to

In the reaction : S + 3/2 O₂ → SO₃ + 2x kcal and SO₂ + 1/2 O₂ → SO₃ + y kcal, heat of formation of SO₂ in kcal is

Formation of ammonia is shown by the reaction, N₂(g) + 3H₂(g) → 2NH₃(g); ΔH° = -91.8 kJ mol⁻¹. What will be the enthalpy of reaction for the decomposition of NH₃ according to the reaction? 2NH₃(g) → N₂(g) + 3H₂(g); ΔH° = ?

Which of the following relationship is not correct?

The enthalpy of solution of sodium chloride is 4 kJ mol⁻¹ and its enthalpy of hydration of ions is 784 kJ mol⁻¹. What will be the lattice enthalpy of sodium chloride?

Match the column I with column II and mark the appropriate choice Column-I (A) CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O (B) H₂(g) → 2H(g) (C) NaCl(s) → Na⁺(g) + Cl⁻(g) (D) NaCl(s) → Na⁺(aq) + Cl⁻(aq) Column-II (i) solH° (ii) latticeH° (iii) cH° (iv) bondH°

The total entropy change (ΔSₜₒₜₐₗ) for the system and surrounding of a spontaneous process is given by

Which of the following expressions regarding entropy is not correct?

Match the column I with column II and mark the appropriate choice

Which of the following statements regarding Gibbs’s energy change is correct?

One word answer is given for the following definitions. Mark the one which is incorrect.

For a reaction, 2K(g) + L(g) → 2M(g); ΔU° = −10.5 kJ and ΔS° = −44.1 J K⁻¹. Calculate ΔG° for the reaction and predict whether the reaction will be spontaneous or non-spontaneous?

Match the columns with and mark the appropriate choice.

A reaction is at equilibrium at 100°C and the enthalpy change for the reaction is 42.6 kJ mol⁻¹. What will be the value of ΔS in J K⁻¹ mol⁻¹?

For an endothermic reaction, ΔH represents the enthalpy of the reaction in kJ mol⁻¹. The minimum amount of activation energy will be:

Which is the correct relationship between ΔG° and equilibrium constant Kₚ?

Match the column I with column II and mark the appropriate choice.

In an adiabatic process, no transfer of heat takes place between system and surroundings. Choose the correct option for free expansion of an ideal gas under adiabatic condition from the following.

The entropy change can be calculated by using the expression, ΔS = -q_rev/T. When water freezes in a glass beaker, choose the correct statement amongst the following.

Consider the reactions given below. On the basis of these reactions find out which of the algebraic relations given in options (a) to (d) is correct? (i) C_(g) + 4H_(g) → CH₄(g); Δ_rH = x kJ mol⁻¹ (ii) C_(graphite, s) + 2H₂(g) → CH₄(g); Δ_rH = y kJ mol⁻¹

The enthalpies of elements in their standard states are taken as zero. The enthalpy of formation of a compound

Enthalpy of sublimation of a substance is equal to

Which of the following graphs represents exothermic reaction?

Which of the following relation is not correct?

The incorrect expression among the following is

For the reaction, 2Cl₍g₎ → Cl₂₍g₎, the correct option is

Which one among the following is the correct option for right relationship between Cₚ and Cᵥ for one mole of ideal gas?

For irreversible expansion of an ideal gas under isothermal condition, the correct option is

Under isothermal conditions, a gas at 30 K expands from 0.1 L to 0.25 L against a constant external pressure of 2 bar. The work done by the gas is [Given that 1 L bar = 100 J]

A gas is allowed to expand in a well insulated container against a constant external pressure of 2.5 atm from an initial volume of 2.50 L to a final volume of 4.50 L. The change in internal energy ΔU of the gas in joules will be

Gas at 27°C temperature and 30 atmospheric pressure is allowed to expand to the spherical pressure. If the volume becomes 10 times its initial volume then the final temperature becomes.

The work done (in ergs) for the reversible expansion of one mole of an ideal gas from a volume of 10 L to 20 L at 25°C is

Among the following, the set of parameters that represents path function, is (A) q + w (B) q (C) w (D) H − TS

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