Thermodynamics Test

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Thermodynamics Test - 36

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Weekly Quiz Competition

Question 1
4 / -1

For a reversible reaction,
X (g) + 3Y (g) ⇌ 2Z(g); ∆H = - 40 kJ, the standard entropies of X ,Y and Z are 60, 40 and 50 JK^-1 mol^-1 respectively. The temperature at which the above reaction attains equilibrium is about

A
400 K

B
500 K

C
273 k

D
373 k
Question 2
4 / -1

The decomposition of limestone
CaCO₃ (g) ⇌ CaO(s) + CO₂ (g)
is non-spontaneous at 298 K. The ∆H° and ∆S° values for the reaction are 76.0 kJ and 60 JK^-1 respectively. At what temperature the decomposition becomes spontaneous ?

A
At 1000 K

B
Below 500° C

C
Between 500° C and 600° C

D
Above 827°C
Question 3
4 / -1

Identify the correct statement regarding a spontaneous process.

A
For a spontaneous process in an isolated system, the change in entropy is positive

B
Endothermic processes are never spontaneous

C
Exothermic processes are always spontaneous

D
Lowering of energy in the reaction process is the only criterion for spontaneity
Question 4
4 / -1

In conversion of limestone to lime,
CaCO₃ (s) → CaO(s) + CO₂ (g )
the values of ∆H° and ∆S °are + 179.1 kJ mol^-1 and 160.2 J/K respectively at 298 K and 1 bar. Assuming that ∆H° and ∆S ° do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is

A
1008 K

B
1200 K

C
845 K

D
1118 K
Question 5
4 / -1

Standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 K are - 382.64 kJ mol^-1 and - 145.6 JK^-1mol^-1, respectively. Standard Gibbs energy change for the same reaction at 298 K is

A
- 2221.1 kJ mol^-1

B
- 339.3 kJ mol^-1

C
- 439.3 kJ mol^-1

D
- 523.2 kJ mol^-1
Question 6
4 / -1

Which of the following is correct for the reaction ∆H = +ve and ∆S = +ve?

A
Spontaneous at high temperature

B
Spontaneous at low temperature

C
Non-spontaneous at high temperature

D
Non-spontaneous at all temperatures
Question 7
4 / -1

What is the relation between E° and K ?

A

B

C

D
Question 8
4 / -1

A schematic plot of In K_eq versus inverse of temperature for a reaction is shown below

A
highly spontaneous at ordinary temperature

B
one with negligible enthalpy change

C
endothermic

D
exothermic
Question 9
4 / -1

The enthalpy change for the transition of liquid water to steam is 40.8 kJ per mol at 100°C. The entropy change for the process will be

A
0.408 JK^-1 mol^-1

B
408 JK^-1 mol^-1

C
109.4 JK^-1 mol^-1

D
0.1094 JK^-1 mol^-1
Question 10
4 / -1

If an endothermic reaction is non-spontaneous at freezing point of water and becomes feasible at its boiling point, then

A
∆H is -ve, ∆S is +ve

B
∆H and ∆S both are +ve

C
∆H and ∆S both are -ve

D
∆H is +ve, ∆S is -ve