11th Chemistry Monthly Test - 2 ( Thermodynamics )

MABS Institution

11th Chemistry Monthly Test - 2 ( Thermodynamics )-Aug 2020

Time : 2.30 Hours

Part - A

Multiple Choice Question - Answer All Question

The gravitational work done by an object is -------

The SI unit of heat is--------

Joule
Calorie
mole
J mol^-1

-----is an intensive property

internal energy
volume
temperature
mass

An ideal gas expands from the volume of 1 x 10^-3 m³to 1 x 10^-2m³ at 300 K against a constant pressure at 1 x 10⁵ Nm^-2. The work done is

- 900 J
900 kJ
270 kJ
-900 kJ

The enthalpy and entropy change for a chemical reactions are -5.3 x 10³ cal and 4.7 cal K^-1 respectively. Predict the nature of the reaction at 298 k.

Non feasible
Reversible
Non-spontaneous
Spontaneous

The amount of heat exchanged with the surrounding at constant temperature pressure is given by the quantity

If one mole of ammonia and one mole of hydrogen chloride are mixed in a closed container to form ammonium chloride gas, then

ΔH > ΔU
ΔH - ΔU = 0
ΔH + ΔU = 0
ΔH < ΔU

In a reversible process, the change in entropy of the universe is

Molar heat of vapourization of a liquid is 4.8 kJ mol-1. If the entropy change is 16 J mol^-1 K^-1, the boiling point of the liquid is

323 K
27° C
164 K
0.3 K

In an endothermic reaction, the value of ΔH is always

=0
>0
<0
constant

Part - B

Generic 2 - Answer All Question

Give Kelvin statement of second law of thermodynamics.

State the first law of thermodynamics.

Define the calorific value of food. What is the unit of calorific value?

Define molar heat capacity. Give its unit
What is lattice energy?

Define enthalpy of neutralization

State the third law of thermodynamics.

Part - C

Generic 3 - Answer All Question

Define enthalpy.

What is absolute zero temperature?

Define entropy of vapourisation.

State zeroth law of thermodynamics.
Predict the sign of entropy change in each of the following:
(i) A liquid crystallises into solid.
(ii) C (graphite) ⟶ C (Diamond)
(iii) Temperature of perfectly crystalline solid is raised from 0K to 115 K.
(iv) AgNO_3(s) ⟶ AgNO_3(aq)

Calculate the enthalpy of hydrogenation of ethylene from the following data. Bond energies of C - H, C - C , C = C and H - H are 414, 347, 618 and 435 kJ mol^-1

State the various statements of second law of thermodynamics.

Part - D

Generic 5 - Answer All Question

The heat of combustion of solid naphthalene (C₁₀H₁₀) at constant volume was -4984 kJ mol^-1at 298 K. Calculate the value of enthalpy change.
Given:
C₁₀H_8(s)+12O_2(g)➝ 10CO_2(g)+4H₂O(l)
\(\Delta U\)=-4984 kJ mol^-1
\(\Delta U\)=-4984 kJ mol^-1,R=8.314 JK^-1 mol^-1
T=298 K

Explain how heat absorbed at constant volume is measured using bomb calorimeter with a neat diagram.

Calculate the enthalpy change for the reaction
Fe₂O₃ + 3CO ⟶ 2Fe + 3CO₂ from the following data.
2Fe +\(\frac{3}{2}\)O₂ ⟶ Fe₂O₃; ΔH = -741 kJ
C +\(\frac{1}{2}\)O₂ ⟶ CO; ΔH = -137 kJ
C + O₂ ⟶ CO₂; ΔH = - 394.5 kJ

Calculate the entropy change when 1 mole of ethanol is evaporated at 351 K The molar heat of vaporisation of ethanol is 39.84 kJ mol^-1.

Calculate the heat of glucose and its calorific value from following data:
(i) C_(graphite)+O_2(g) ➝ CO_2(g); ΔH= -395 KJ
(ii) H_2(g)+\(\frac{1}{2}\)O₂ ➝ H₂O_(l); ΔH= -269.4 KJ
(iii) C+6H_2(g)+3O_2(g) ➝ C₆H₁₂O_6(s); ΔH= -1169.8 KJ

If an automobile engine burns petrol at a temperature of 816° C and if the surrounding temperature is 21° C, calculate its maximum possible efficiency

Calculate the standard free energy change \(({ \Delta G }^{ o })\) of the following reaction and say whether it is feasible at 373 K or not.\(\frac{1}{2}H_{2(g)}+\frac{1}{2}I_{2(g)} \rightarrow HI_{(g)}\) \({ \Delta H }_{ r }^{ o }\) is + 25.95 kJ mol^-1 standard entropies of HI_(g) H_2(g) and I_2(g) are 206.3,140.6 and 118.7 Jk^-1 mol-1.

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11th Chemistry Monthly Test - 2 ( Thermodynamics )

MABS Institution

11th Chemistry Monthly Test - 2 ( Thermodynamics )-Aug 2020

Part - A

Multiple Choice Question - Answer All Question

The gravitational work done by an object is -------

The SI unit of heat is--------

-----is an intensive property

An ideal gas expands from the volume of 1 x 10-3 m3 to 1 x 10-2 m3 at 300 K against a constant pressure at 1 x 105 Nm-2. The work done is

The enthalpy and entropy change for a chemical reactions are -5.3 x 103 cal and 4.7 cal K-1 respectively. Predict the nature of the reaction at 298 k.

The amount of heat exchanged with the surrounding at constant temperature pressure is given by the quantity

If one mole of ammonia and one mole of hydrogen chloride are mixed in a closed container to form ammonium chloride gas, then

In a reversible process, the change in entropy of the universe is

Molar heat of vapourization of a liquid is 4.8 kJ mol-1. If the entropy change is 16 J mol -1 K-1, the boiling point of the liquid is

In an endothermic reaction, the value of ΔH is always

Part - B

Generic 2 - Answer All Question

Give Kelvin statement of second law of thermodynamics.

State the first law of thermodynamics.

Define the calorific value of food. What is the unit of calorific value?

Define molar heat capacity. Give its unit

What is lattice energy?

Define enthalpy of neutralization

State the third law of thermodynamics.

Part - C

Generic 3 - Answer All Question

Define enthalpy.

What is absolute zero temperature?

Define entropy of vapourisation.

State zeroth law of thermodynamics.

Predict the sign of entropy change in each of the following: (i) A liquid crystallises into solid. (ii) C (graphite) ⟶ C (Diamond) (iii) Temperature of perfectly crystalline solid is raised from 0K to 115 K. (iv) AgNO3(s) ⟶ AgNO3(aq)

Calculate the enthalpy of hydrogenation of ethylene from the following data. Bond energies of C - H, C - C , C = C and H - H are 414, 347, 618 and 435 kJ mol-1

State the various statements of second law of thermodynamics.

Part - D

Generic 5 - Answer All Question

The heat of combustion of solid naphthalene (C10H10) at constant volume was -4984 kJ mol-1 at 298 K. Calculate the value of enthalpy change. Given: C10H8(s)+12O2(g) ➝ 10CO2(g)+4H2O(l) \(\Delta U\)=-4984 kJ mol-1 \(\Delta U\)=-4984 kJ mol-1,R=8.314 JK-1 mol-1 T=298 K

Explain how heat absorbed at constant volume is measured using bomb calorimeter with a neat diagram.

Calculate the enthalpy change for the reaction Fe2O3 + 3CO ⟶ 2Fe + 3CO2 from the following data. 2Fe +\(\frac{3}{2}\)O2 ⟶ Fe2O3; ΔH = -741 kJ C +\(\frac{1}{2}\)O2 ⟶ CO; ΔH = -137 kJ C + O2 ⟶ CO2; ΔH = - 394.5 kJ

Calculate the entropy change when 1 mole of ethanol is evaporated at 351 K The molar heat of vaporisation of ethanol is 39.84 kJ mol-1.

Calculate the heat of glucose and its calorific value from following data: (i) C(graphite)+O2(g) ➝ CO2(g); ΔH= -395 KJ (ii) H2(g)+\(\frac{1}{2}\)O2 ➝ H2O(l); ΔH= -269.4 KJ (iii) C+6H2(g)+3O2(g) ➝ C6H12O6(s); ΔH= -1169.8 KJ

If an automobile engine burns petrol at a temperature of 816° C and if the surrounding temperature is 21° C, calculate its maximum possible efficiency

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An ideal gas expands from the volume of 1 x 10^-3 m³to 1 x 10^-2m³ at 300 K against a constant pressure at 1 x 10⁵ Nm^-2. The work done is

The enthalpy and entropy change for a chemical reactions are -5.3 x 10³ cal and 4.7 cal K^-1 respectively. Predict the nature of the reaction at 298 k.

Molar heat of vapourization of a liquid is 4.8 kJ mol-1. If the entropy change is 16 J mol^-1 K^-1, the boiling point of the liquid is

Predict the sign of entropy change in each of the following:
(i) A liquid crystallises into solid.
(ii) C (graphite) ⟶ C (Diamond)
(iii) Temperature of perfectly crystalline solid is raised from 0K to 115 K.
(iv) AgNO_3(s) ⟶ AgNO_3(aq)

Calculate the enthalpy of hydrogenation of ethylene from the following data. Bond energies of C - H, C - C , C = C and H - H are 414, 347, 618 and 435 kJ mol^-1

The heat of combustion of solid naphthalene (C₁₀H₁₀) at constant volume was -4984 kJ mol^-1at 298 K. Calculate the value of enthalpy change.
Given:
C₁₀H_8(s)+12O_2(g)➝ 10CO_2(g)+4H₂O(l)
\(\Delta U\)=-4984 kJ mol^-1
\(\Delta U\)=-4984 kJ mol^-1,R=8.314 JK^-1 mol^-1
T=298 K

Calculate the enthalpy change for the reaction
Fe₂O₃ + 3CO ⟶ 2Fe + 3CO₂ from the following data.
2Fe +\(\frac{3}{2}\)O₂ ⟶ Fe₂O₃; ΔH = -741 kJ
C +\(\frac{1}{2}\)O₂ ⟶ CO; ΔH = -137 kJ
C + O₂ ⟶ CO₂; ΔH = - 394.5 kJ

Calculate the entropy change when 1 mole of ethanol is evaporated at 351 K The molar heat of vaporisation of ethanol is 39.84 kJ mol^-1.

Calculate the heat of glucose and its calorific value from following data:
(i) C_(graphite)+O_2(g) ➝ CO_2(g); ΔH= -395 KJ
(ii) H_2(g)+\(\frac{1}{2}\)O₂ ➝ H₂O_(l); ΔH= -269.4 KJ
(iii) C+6H_2(g)+3O_2(g) ➝ C₆H₁₂O_6(s); ΔH= -1169.8 KJ