Important Questions of Thermodynamics Chemistry | Zigya

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101.

What is the amount of work done when 0.5 mole of methane, CH4(g), is subjected to combustion at 300 K? (Given, R=8.314JK-1 mol-1)

  • -2494 J

  • -4988 J

  • + 4988 J

  • + 2494 J


102.

In the reaction; A2(g) + 3B2(g) → 2AB3(g), the standard entropies in (JK-1 mol-1) of A2(g), B2(g) and AB3(g) are respectively 190, 130 and 195 and the standard enthalpy change for the reaction is -95 kJ mol-1. The temperature (in K) at which the reaction attains equilibrium is (assuming both the standard entropy change and standard enthalpy change for this reaction are constant over a wide range of temperature)

  • 500

  • 400

  • 300

  • 200


103.

Calculate the standard enthalpy change (in kJ mol-1) for the reaction

    H2(g) + O2(g) → H2O2(g)

Given that bond enthalpies of H-H, O=O, O-H and O-O (in KJ mol-1) are respectively 438, 498, 464 and 138.

 

  • -130

  • -65

  • +130

  • -334


104.

According to the first law of thermodynamics which of the following quantities represents the change in a state function?

  • qrev + Wrev

  • qrev

  • qrev - Wrev

  • qrev / Wrev


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105.

If the activation energy for the forward reaction is 150 kJ mol-1 and that of the reverse reaction is 260 kJ mol-1, what is the enthalpy change for the reaction?

  • 410 kJ mol-1

  • 110kJ mol-1

  • -110 kJ mol-1

  • -410 kJ mol-1


106.

When 0.2 g of 1-butanol was burnt in a suitable apparatus, the heat evolved was sufficient to raise the temperature of 200 g water by 5°C. The enthalpy of combustion of 1-butanol in kcal mol-1 will be

  • +37

  • +370

  • -370

  • -740


107.

Given that dE = Tds - pdV and H = E + pV. Which one of the following relations is true ?

  • dH = TdS + Vdp

  • dH = SdT + Vdp

  • dH = -SdT + Vdp

  • dH = dE + pdV


108.

Using the following thermochemical equations

(i) S(rh) + 3/2O2(g) → SO3 (g)       ΔH = -2x kJ mol-1

(ii) SO2(g) + 1/2O2 (g)  → SO3 (g)  ΔH = -y kJ mol-1

Find out the heat of formation of SO2 (g) in kJ mol-1.

  • (2x + y)

  • (x + y)

  • (2x/y)

  • (y- 2x)


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109.

The activation energy of exothermic reaction A → B is 80 kJ mo1-1. The heat of reaction is 200 kJ mol-1. The activation evergy for the reaction B → A (in kJ mol-1) will be

  • 280

  • 200

  • 120

  • 40


110.

What would be the heat released when an aqueous solution containing 0.5 mole of HNO3 is mixed with 0.3 mole of OH- (enthalpy of neutralization is -57.1 k.J) ?

  • 28.5 kJ

  • 17.1 kJ

  • 45.7 kJ

  • 1.7 kJ


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