11th Chemistry Thermodynamics Model Question Paper | QB365

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11th Chemistry Thermodynamics Model Question Paper

Published on: 20/08/2019

Thermodynamics

Download Tamil Nadu 11th Standard Chemistry question papers, model tests, one-mark questions, important questions, and public exam papers in PDF format. Free study materials and answer keys for TN State Board students.

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Std: 11th Standard - Chemistry

chapter: - Model Question paper

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Questions:

Multiple Choice Question

10 x 1 = 10

Heat absorbed at constant volume is measured in ____________ calorimeter.

(a)

Coffee cup

(b)

Differential scanning

(c)

Bomb

(d)

Adiabatic

ΔH^o of H₂O₍₁₎is KJ/mol.

(a)

-74.85

(b)

-242

(c)

+242

(d)

+74.85

In a compression process, P_ext is ___________

(a)

(P_int+ dP)

(b)

(P_int- dP)

(c)

(dP-P_int)

(d)

(-P_int+dP)

Which among the following is a state function?

(a)

Pressure

(b)

Enthalpy

(c)

Heat

(d)

Both (a) and (b)

Which among the following is not a state function?

(a)

Pressure

(b)

Volume

(c)

Temperature

(d)

Work

Which among the following is not an extensive property?

(a)

Volume

(b)

internal energy

(c)

Mass

(d)

temperature

The bond dissociation energy of methane and ethane are 360 kJ mol^-1 and 620 kJ mol^-1 respectively. Then, the bond dissociation energy of C-C bond is ______________.

(a)

170 kJ mol^-1

(b)

50 kJ mol^-1

(c)

80 kJ mol^-1

(d)

220 kJ mol^-1

Change in internal energy, when 4 kJ of work is done on the system and 1 kJ of heat is given out by the system is ______________

(a)

+1 kJ

(b)

- 5 kJ

(c)

+3 kJ

(d)

- 3 kJ

Heat of combustion is always ____________

(a)

positive

(b)

negative

(c)

zero

(d)

either positive or negative

10.

All the naturally occurring processes proceed spontaneously in a direction which leads to _______________

(a)

decrease in entropy

(b)

increase in enthalpy

(c)

increase in free energy

(d)

decrease in free energy

Generic 2

5 x 2 = 10

11.

Explain Zeroth law of thermodynamics.

12.

Give examples for extensive and intensive properties.

13.

Identify the state and path function out of the following:
a) Enthalpy
b) Entropy
c) Heat
d) Temperature
e) Work
f) Free energy.

14.

Define Gibbs' free energy.

15.

State the first law of thermodynamics.

Generic 3

5 x 3 = 15

16.

Which law of thermodynamics deals with equivalence of different forms of energies?

17.

In the equation N_2(g)+ 3H_2(g) ⇌2NH_3(g) What would be the sign of work done?

18.

For a reaction, 2Cl_(g) ⟶ Cl₂, What are the signs of ΔH and ΔS?

19.

In a constant volume calorimeter:3.5g of a gas with molecular weight 28 was burnt in excess oxygen at 298 K. The temperature of the calorimeter was found to increase from 298 K to 298.45 K due to the combustion process. Given that the calorimeter constant is 2.5 kJ K^-1. Calculate the enthalpy of combustion of the gas in kJ mol^-1

20.

What are state and path functions? Give two examples

Generic 5

2 x 5 = 10

21.

For the equilibrium \({ PCl }_{ 5 }\rightleftharpoons { PCl }_{ 3(g) }+{ Cl }_{ 2(g) }\) at 298 K, K is 1.8 x 10^-7. What is the ΔG⁰ for the reaction?

22.

List the characteristics of internal energy.

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Answers Key:

Multiple Choice Question

10 x 1 = 10

(b)
-242

(a)
(P_int+ dP)

(d)
Both (a) and (b)

(d)
Work

(d)
temperature

(b)
negative

10.

(d)
decrease in free energy

Generic 2

5 x 2 = 10

11.

According to this law, if systems Band C separately are in thermal equilibrium with another system A, then systems Band C will also be in thermal equilibrium with each other. This is also the principle by which thermometers are used.

12.

Extensive properties	Intensive properties
volume, mass, amount of substance. (mole), energy, enthalpy, entropy, free energy, heat capacity.	molar volume, density, molar mass, molarity mole fraction, molality, specific heat capacity.

13.

State Function: Enthalpy, entropy, temperature, free energy
Path Function: Heat, work.

14.

Gibbs free energy is defined as G = H - TS

15.

The first law of thermodynamics, also known as the law of conservation of energy, states that "The total energy of an isolated system remains constant though it may change from one form to another."
The mathematical statement of the First Law is: ΔU=q+w
Where q - the amount of heat supplied to the system; w - work done on the system

Generic 3

5 x 3 = 15

16.

First law of Thermodynamics.

17.

Work is done on the system due to decrease in volume so the sign of work done will be +ve.

18.

The given reaction represents the formation of bonds. Hence energy is released, ie. ΔH is -ve.
Further two moles of atoms will have greater randomness than one mole of molecules. Hence randomness increases so ΔS = +ve.

19.

T_i= 298 K
T_f = 298.45 K
k = 2.5 kJK^-1
m =3.5g
M_m = 28
heat evolved= kΔT
=k (T_f - T_i)
=2.5 KJ K^-1 (298.45 - 298)K
=1.125kJ
ΔH_c=\(\frac{1.125}{3.5}\times\)28KJmol^-1
ΔH_c = 9 kJ mol^-1

20.

(i) State function: A state function is a thermodynamic property of a system, which has a specific value for a given state and does not depend on the path (or manner) by which the particular state is reached.
Example: Pressure (P), Volume (V), Temperature(T)
(ii) Path functions: A path function is a thermodynamic property of the system whose value depends on the path by which the system changes from its initial to final states.
Example: Work (w), Heat (q).

Generic 5

2 x 5 = 10

21.

Given:
R=8.314 JK^-1mol^-1
T=278K
K=1.8 x 10^-7
ΔG⁰=-2.303 RT log K
ΔG⁰=-2.303 x 8.314 x log(1.8 x 10^-7)
ΔG⁰=-2.303 x 8.314 x 298 x (-6.745)
ΔG⁰=38484 J mol^-1
ΔG⁰=38.484 KJ mol^-1.

22.

Characteristics of internal energy (U) :

The internal energy of a system is an extensive property.
The internal energy of a system is a state function.
The change in internal energy of a system is expressed as ΔU= U_f- U_i
In a cyclic process,' there is no internal energy change. ΔU_(cyclic)= 0
If the internal energy of the system in the final state (U_f) is less than the internal energy of the system in its initial state (U_i), then ΔU would be negative.
ΔU = U_f- Ui = -ve (U_f< U_i)
If the internal energy of the system in the final state (U_f) is greater than the internal energy of the system in its initial state (U_i), then ΔU would be positive.
ΔU = U_f- U_i = +ve (U_f> U_i)