Thermodynamics - 2 - Free MCQ Test with solutions for JEE Chemistry

-22.98 JK^-1

22.98 JK^-1

57.4 JK^-1

80.42 JK^-1

0.335 JK^-1

-0.33 JK^-1

0.670 JK^-1

0.00 JK^-1

1.474 bar

0.678 bar

0.796 bar

1.00 bar

ΔS_(System) > 0, ΔS_{(surrounding)} > 0

ΔS_(System) > 0, ΔS_{(surrounding)} < 0

ΔS_(System) < 0, ΔS_{(surrounding)} > 0

ΔS_(System) < 0, ΔS_{(surrounding)} < 0

ΔG is positive

ΔS_(system) is positive

ΔS_{(Surrounding)} is zero

ΔH = 0

(2x + y)

(x – y)

(x + y)

(2x – y)

ΔS_system > 0 and ΔS_surroundings > 0

ΔS_system > 0 and ΔS_surroundings < 0

ΔS_system < 0 and ΔS_surroundings > 0

ΔS_system < 0 and ΔS_surroundings < 0

+10.3 kJ

-43.3 kJ

-10.3 kJ

+6.2 kJ

-261 kJ

+103 kJ

+261 kJ

-103 kJ

C is the thermodynamically stable product.

Formation of A and B from C has highest enthalpy of activation.

Activation enthalpy to form C is 5 kJ mol^–1 less than that to form D

D is kinetically stable product.

(A), (B) and (C)

(B) and (C)

(A) and (D)

(B), (C) and (D)

8

9

10

11

+141.2 kJ/mol

+1412 kJ/mol

–141.2 kJ/mol

–1412 kJ/mol

Adiabatic process : ΔU = –w

Cyclic process : q = – w

Isothermal process : q = – w

Isochoric process : ΔU = q

5

10

95

100

1250 K

500 K

750 K

1000 K

2.85

22.8

11.4

5.7

–6 J

–608 J

+304 J

–304 J