NCERT Exemplar solutions for Chemistry [English] Class 11 chapter 6 - Thermodynamics [Latest edition]

Thermodynamics is not concerned about ______.

Which of the following statements is correct?

The state of a gas can be described by quoting the relationship between ______.

The volume of gas is reduced to half from its original volume. The specific heat will be ______.

During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for above change is ______.

\[\ce{∆_f U^Θ}\] of formation of \[\ce{CH4 (g)}\] at certain temperature is – 393 kJ mol^–1. The value of \[\ce{∆_f H^Θ}\] is ______.

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 pressure-volume work for an ideal gas can be calculated by using the expression w = `- int_(v_i)^(v_f) p_(ex)  dV`. The work can also be calculated from the pV– plot by using the area under the curve within the specified limits. When an ideal gas is compressed (a) reversibly or (b) irreversibly from volume V_i to V_f. choose the correct option.

The entropy change can be calculated by using the expression ∆S = `q_(rev)/T`. When water freezes in a glass beaker, choose the correct statement amongst the following :

On the basis of thermochemical equations (a), (b) and (c), find out which of the algebric relationships given in options (i) to (iv) is correct.

(a) \[\ce{C (graphite) + O2 (g) -> CO2 (g) ; ∆_rH = xkJ mol^{-1}}\]

(b) \[\ce{C (graphite) + 1/2 O2 (g) -> CO (g) ; ∆_rH = ykJ mol^{-1}}\]

(c) \[\ce{CO (g) + 1/2 O2 (g) -> CO2 (g) ; ∆_r H = zkJ mol^{-1}}\]

Consider the reactions given below. On the basis of these reactions find out which of the algebric relations given in options (i) to (iv) is correct?

(a) \[\ce{C (g) + 4 H (g) -> CH4 (g); ∆_rH = xkJ mol^{-1}}\]

(b) \[\ce{C (graphic) + 2H2 (g) -> CH4 (g); ∆_rH = ykJ mol^{-1}}\]

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 is not correct?

Thermodynamics mainly deals with:

(i) interrelation of various forms of energy and their transformation from one form to another.

(ii) energy changes in the processes which depend only on initial and final states of the microscopic systems containing a few molecules.

(iii) how and at what rate these energy transformations are carried out.

(iv) the system in equilibrium state or moving from one equilibrium state to another equilibrium state.

In an exothermic reaction, heat is evolved, and system loses heat to the surrounding. For such system:

(i) q_p will be negative

(ii) ∆_rH will be negative

(iii) q_p will be positive

(iv) ∆_rH will be positive

The spontaneity means, having the potential to proceed without the assistance of external agency. The processes which occur spontaneously are:

(i) Flow of heat from colder to warmer body.

(ii) Gas in a container contracting into one corner.

(iii) Gas expanding to fill the available volume.

(iv) Burning carbon in oxygen to give carbon dioxide.

For an ideal gas, the work of reversible expansion under isothermal condition can be calculated by using the expression w = `- nRT` In `V_f/V_i`. A sample containing 1.0 mol of an ideal gas is expanded isothermally and reversibly to ten times of its original volume, in two separate experiments. The expansion is carried out at 300 K and at 600 K respectively.

(i) Work done at 600 K is 20 times the work done at 300 K.

(ii) Work done at 300 K is twice the work done at 600 K.

(iii) Work done at 600 K is twice the work done at 300 K.

(iv) ∆U = 0 in both cases.

Consider the following reaction between zinc and oxygen and choose the correct options out of the options given below:

\[\ce{2 Zn (s) + O2 (g) -> 2 ZnO (s); ∆H = - 693.8 kJ mol^{-1}}\]

(i) The enthalpy of two moles of \[\ce{ZnO}\] is less than the total enthalpy of two moles of \[\ce{Zn}\] and one mole of oxygen by 693.8 kJ.

(ii) The enthalpy of two moles of \[\ce{ZnO}\] is more than the total enthalpy of two moles of \[\ce{Zn}\] and one mole of oxygen by 693.8 kJ.

(iii) 693.8 kJ mol^–1 energy is evolved in the reaction.

(iv) 693.8 kJ mol^–1 energy is absorbed in the reaction.

18.0 g of water completely vapourises at 100°C and 1 bar pressure and the enthalpy change in the process is 40.79 kJ mol–1. What will be the enthalpy change for vapourising two moles of water under the same conditions? What is the standard enthalphy of vapourisation for water?

One mole of acetone requires less heat to vapourise than 1 mol of water. Which of the two liquids has higher enthalpy of vapourisation?

Standard molar enthalpy of formation, ∆_fH^Θ is just a special case of enthalpy of reaction, ∆_rH^Θ. Is the ∆_rH^Θ for the following reaction same as ∆_fH^Θ? Give reason for your answer.

\[\ce{CaO(s) + CO2(g) -> CaCO3(s); ∆_fH^Θ = - 178.3 kJ mol^{-1}}\]

The value of ∆_fH^Θ for \[\ce{NH3}\] is – 91.8 kJ mol^–1. Calculate enthalpy change for the following reaction:

\[\ce{2NH3(g) -> N2(g) + 3H2(g)}\]

Enthalpy is an extensive property. In general, if enthalpy of an overall reaction A→B along one route is ∆_rH and ∆_rH₁, ∆_rH₂, ∆_rH₃ ..... represent enthalpies of intermediate reactions leading to product B. What will be the relation between ∆_rH for overall reaction and ∆_rH₁, ∆_rH₂ ..... etc. for intermediate reactions.

The enthalpy of atomisation for the reaction \[\ce{CH4(g) -> C(g) + 4H(g)}\] is 1665 kJ mol^–1. What is the bond energy of \[\ce{C – H}\] bond?

Use the following data to calculate \[\ce{∆_{lattice}H^Θ}\] for \[\ce{NaBr}\].

\[\ce{∆_{sub}H^Θ}\] for sodium metal = 108.4 kJ mol^–1

Ionization enthalpy of sodium = 496 kJ mol^–1

Electron gain enthalpy of bromine = – 325 kJ mol^–1

Bond dissociation enthalpy of bromine = 192 kJ mol^–1

\[\ce{∆_fH^Θ}\] for \[\ce{NaBr (s)}\] = – 325 kJ mol^–1 

Given that ∆H = 0 for mixing of two gases. Explain whether the diffusion of these gases into each other in a closed container is a spontaneous process or not?

Heat has randomising influence on a system and temperature is the measure of average chaotic motion of particles in the system. Write the mathematical relation which relates these three parameters.

Increase in enthalpy of the surroundings is equal to decrease in enthalpy of the system. Will the temperature of system and surroundings be the same when they are in thermal equilibrium?

At 298 K. K_p for the reaction \[\ce{N2 O4 (g) ⇌ 2NO2 (g)}\] is 0.98. Predict whether the reaction is spontaneous or not.

A sample of 1.0 mol of a monoatomic ideal gas is taken through a cyclic process of expansion and compression as shown in figure 6.1. What will be the value of ∆H for the cycle as a whole?

The standard molar entropy of \[\ce{H2O (l)}\] is 70 JK^–1 mol^–1. Will the standard molar entropy of \[\ce{H2O (s)}\] be more, or less than 70 JK^–1 mol^–1?

Identify the state and path functions out of the following:

1. Enthalpy
2. Entropy
3. Heat
4. Temperature
5. Work
6. Free energy

The molar enthalpy of vapourisation of acetone is less than that of water. Why?

Which quantity out of ∆_rG and ∆_rG^Θ will be zero at equilibrium?

Predict the change in internal energy for an isolated system at constant volume.

Although heat is a path function but heat absorbed by the system under certain specific conditions is independent of path. What are those conditions? Explain.

Expansion of a gas in vacuum is called free expansion. Calculate the work done and the change in internal energy when 1 litre of ideal gas expands isothermally into vacuum until its total volume is 5 litre?

Heat capacity (C_p) is an extensive property but specific heat (c) is an intensive property. What will be the relation between C_p and c for 1 mol of water?

The difference between C_P and C_V can be derived using the empirical relation H = U + pV. Calculate the difference between C_P and C_V for 10 moles of an ideal gas.

If the combustion of 1g of graphite produces 20.7 kJ of heat, what will be molar enthalpy change? Give the significance of sign also.

The net enthalpy change of a reaction is the amount of energy required to break all the bonds in reactant molecules minus amount of energy required to form all the bonds in the product molecules. What will be the enthalpy change for the following reaction.

\[\ce{H2(g) + Br(g) -> 2HBr(g)}\]

Given that Bond energy of \[\ce{H2, Br2}\] and \[\ce{HBr}\] is 435 kJ mol^–1, 192 kJ mol^–1 and 368 kJ mol^–1 respectively.

The enthalpy of vapourisation of \[\ce{CCl4}\] is 30.5 kJ mol^–1. Calculate the heat required for the vapourisation of 284 g of \[\ce{CCl4}\] at constant pressure. (Molar mass of \[\ce{CCl4}\] = 154 g mol^–1).

The enthalpy of reaction for the reaction: \[\ce{2H2 (g) + O2(g) -> 2H2O (l)}\] is ∆_rH^Θ = – 572 kJ mol^–1. What will be standard enthalpy of formation of \[\ce{H2O (l)}\]?

What will be the work done on an ideal gas enclosed in a cylinder, when it is compressed by a constant external pressure, p_ext in a single step as shown in figure. Explain graphically.

How will you calculate work done on an ideal gas in a compression, when change in pressure is carried out in infinite steps?

Represent the potential energy/enthalpy change in the following processes graphically.

(a) Throwing a stone from the ground to roof.

(b) \[\ce{1/2 H2(g) + 1/2 Cl2 (g) ⇌ HCl (g) Δ_rH^Θ = - 92.32 kJ mol^{-1}}\]

In which of the processes potential energy/enthalpy change is contributing factor to the spontaneity?

Enthalpy diagram for a particular reaction is given in figure. Is it possible to decide spontaneity of a reaction from given diagram. Explain.

1.0 mol of a monoatomic ideal gas is expanded from state (1) to state (2) as shown in figure. Calculate the work done for the expansion of gas from state (1) to state (2) at 298 K.

An ideal gas is allowed to expand against a constant pressure of 2 bar from 10 L to 50 L in one step. Calculate the amount of work done by the gas. If the same expansion were carried out reversibly, will the work done be higher or lower than the earlier case? (Given that 1 L bar = 100 J)

Match the following :

Match the following processes with entropy change:

Match the following parameters with description for spontaneity 

Match the following :

Assertion (A): Combustion of all organic compounds is an exothermic reaction.

Reason (R): The enthalpies of all elements in their standard state are zero.

Assertion (A): Spontaneous process is an irreversible process and may be reversed by some external agency.

Reason (R): Decrease in enthalpy is a contributory factor for spontaneity.

Assertion (A): A liquid crystallises into a solid and is accompanied by decrease in entropy.

Reason (R): In crystals, molecules organise in an ordered manner.

Derive the relationship between ∆H and ∆U for an ideal gas. Explain each term involved in the equation.

Extensive properties depend on the quantity of matter but intensive properties do not. Explain whether the following properties are extensive or intensive.

The lattice enthalpy of an ionic compound is the enthalpy when one mole of an ionic compound present in its gaseous state, dissociates into its ions. It is impossible to determine it directly by experiment. Suggest and explain an indirect method to measure lattice enthalpy of \[\ce{NaCl(s)}\].

\[\ce{∆G}\] is net energy available to do useful work and is thus a measure of “free energy”. Show mathematically that ∆G is a measure of free energy. Find the unit of \[\ce{∆G}\]. If a reaction has positive enthalpy change and positive entropy change, under what condition will the reaction be spontaneous?

Graphically show the total work done in an expansion when the state of an ideal gas is changed reversibly and isothermally from \[\ce{(p_i, V_i)}\] to \[\ce{(p_f , V_f )}\]. With the help of a pV plot compare the work done in the above case with that carried out against a constant external pressure \[\ce{p_f}\].