Thermodynamics Test

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Thermodynamics Test - 51

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Weekly Quiz Competition

Question 1
4 / -1

AB, A₂ and B₂ are diatomic molecules. If the bond enthalpies of A₂, AB & B₂ are in the ratio 1 : 1 : 0.5 and enthalpy of formation of AB from A₂ and B₂ is – 100 kJ/mol^–1. What is the bond enthalpy of A₂.

A
400 kJ/mol

B
200 kJ/mol

C
100 kJ/mol

D
300 kJ/mol
Question 2
4 / -1

A
298 K

B
668 K

C
966 K

D
∆G° is +ve, hence the reaction will never be spontaneous
Question 3
4 / -1

One mole of a gas occupying 3 dm³ expands against constant external pressure of 1 atm to a volume of 13 dm³. The work done is –

A
– 10 atm dm³

B
– 20 atm dm³

C
– 39 atm dm³

D
– 48 atm dm³
Question 4
4 / -1

The enthalpy change in the oxidation of glucose is – 2880 kJ mol^–1. Twenty five per cent of this energy is available for muscular work. If 100 kJ of muscular work is needed to walk one kilometre, then the maximum distance that a person will be able to walk after eating 120 g of glucose will be

A
4.8 km

B
2.4 km

C
8.4 km

D
9.8 km
Question 5
4 / -1

The heat of formation of liquid methyl alcohol is kilo joule per mole using the following data will be [Heat of vaporisation of liquid methyl alcohol = 38 kJ/mol. Heat of formation of gaseous atoms from the elements in their standard states : H, 218 kJ/mol; C, 715 kJ/mol; O, 249 kJ/mol. Average bond energies : C – H, 415 kJ/mol; C – O, 356 kJ/mol O – H, 463 kJ/mol.]

A
46.0 kJ/mole

B
50.0 kJ/mole

C
73.3 kJ/mole

D
– 266 kJ/mole
Question 6
4 / -1

10 g of argon gas is compressed isothermally and reversibly at a temperature of 27°C from 10 L to 5 L. q, W, ∆E and ∆H for this process are [R = 2.0 cal K–1 mo l–1, log₁₀ 2 = 0.30. [Atomic wt. of Ar = 40.]

A
W = 106.635 cal, q = 103.635 cal, ∆E ≠ 0 & ∆H = 0

B
W = 53.635 cal, q = – 53.635 cal, ∆E ≠ 0 & ∆H = 0

C
W = – 53.635 cal, q = 63.635 cal, ∆E & ∆H ≠ 0

D
W = 103.635 cal, q = – 103.635 cal, ∆E & ∆H = 0
Question 7
4 / -1

Molar heat capacity of water in equilibrium with ice at constant pressure is –

A
zero

B
infinity (∞)

C
40.45 kJ^–1 mol^–1

D
75.48 J K^–1 mol^{– 1}
Question 8
4 / -1

Diborane is a potential rocket fuel which undergoes combustion according to the reaction,
B₂H₆ (g) + 3O₂ (g) → B₂O₃ (s) + 3H₂O(g)
from the following data, the enthalpy change for the combustion of diborane will be
2B(s) + O₂ (g) → B₂O₃(s); ∆H = – 1273 kJ
H₂(g) + O₂ (g) → H₂O(l); ∆H = – 286 kJ
H₂O(l) → H₂O(g) ; ∆H = 44 kJ
2B(s) + 2H₂ (g) → B₂H₆ (g); ∆H = 46 kJ

A
– 2079 kJ mol^–1

B
– 1091 kJ mol^–1

C
– 2035 kJ mol^–1

D
– 762 kJ mol^–1
Question 9
4 / -1

A sample of argon gas at 1 atm pressure and 27°C expands reversibly and adiabatically from 1.25 dm³ to 2.50 dm³. The enthalpy change in this process will be………. [Cv.m. for argon is 12.48 jK^–1 mol^–1].

A
114.52 J

B
– 114.52 J

C
– 57.26 J

D
57.26 J
Question 10
4 / -1

Find ∆G° and ∆H° for that the reaction CO(g) + O₂ (g) → CO₂ (g) at 300 K respectively are, when the standard entropy change is – 0.094 kJ mol^–1 K^–1. The standard Gibbs free energies of formation for CO₂ and CO are – 394.4 and – 137.2 kJ mol^–1, respectively.

A
∆G° = 257.2 kJ/mol, DH° = 285.4 kJ/mol

B
∆G° = 514.4 kJ/mol, DH° = – 570.8 kJ/mol

C
∆G° = +514.4 kJ/mol, DH° = 570.8 kJ/mol

D
∆G° = – 257.2 kJ/mol, DH° = – 285.4 kJ/mol

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Thermodynamics Test - 51

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Thermodynamics Test - 51

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SHARING IS CARING

Question 1

400 kJ/mol

200 kJ/mol

100 kJ/mol

300 kJ/mol

Question 2

298 K

668 K

966 K

∆G° is +ve, hence the reaction will never be spontaneous

Question 3

– 10 atm dm3

– 20 atm dm3

– 39 atm dm3

– 48 atm dm3

Question 4

4.8 km

2.4 km

8.4 km

9.8 km

Question 5

46.0 kJ/mole

50.0 kJ/mole

73.3 kJ/mole

– 266 kJ/mole

Question 6

W = 106.635 cal, q = 103.635 cal, ∆E ≠ 0 & ∆H = 0

W = 53.635 cal, q = – 53.635 cal, ∆E ≠ 0 & ∆H = 0

W = – 53.635 cal, q = 63.635 cal, ∆E & ∆H ≠ 0

W = 103.635 cal, q = – 103.635 cal, ∆E & ∆H = 0

Question 7

zero

infinity (∞)

40.45 kJ–1 mol–1

75.48 J K–1 mol– 1

Question 8

– 2079 kJ mol–1

– 1091 kJ mol–1

– 2035 kJ mol–1

– 762 kJ mol–1

Question 9

114.52 J

– 114.52 J

– 57.26 J

57.26 J

Question 10

∆G° = 257.2 kJ/mol, DH° = 285.4 kJ/mol

∆G° = 514.4 kJ/mol, DH° = – 570.8 kJ/mol

∆G° = +514.4 kJ/mol, DH° = 570.8 kJ/mol

∆G° = – 257.2 kJ/mol, DH° = – 285.4 kJ/mol

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– 10 atm dm³

– 20 atm dm³

– 39 atm dm³

– 48 atm dm³

40.45 kJ^–1 mol^–1

75.48 J K^–1 mol^{– 1}

– 2079 kJ mol^–1

– 1091 kJ mol^–1

– 2035 kJ mol^–1

– 762 kJ mol^–1