Thermodynamics Test

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Thermodynamics Test - 27

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Weekly Quiz Competition

Question 1
1 / -0

In the evaporation of water, the entropy

A
does not change

B
increases

C
decreases

D
first increases and then decreases

Solution

As the randomness increases on evaporation, entropy also increases.
The greater the randomness in a system, greater is its entropy.
Question 2
1 / -0

The value of ΔS for spontaneous process is

A
ΔS_Total is constant

B
ΔS_Total > 0

C
ΔS_Total < 0

D
ΔS_Total = 0

Solution

The second law of thermodynamics states that for any spontaneous process, the overall ΔS must be greater than or equal to zero.
Question 3
1 / -0

What is the change in the entropy of water, When ice melts into water?

A
Entropy of water increases.

B
Entropy of water becomes zero.

C
Entropy of water decreases.

D
Entropy of water remains same.

Solution

The greater the randomness in a system, greater is its entropy. The randomness is greater in liquid state as compared to solid state so the entropy increases when ice melts into water.
Question 4
1 / -0

For the reaction Hg (l) ———> Hg (g) , the entropy change will have the sign:

A
Negative

B
Positive

C
Both positive and negative

D
None of the above

Solution

In this reaction, disordered gaseous state changes to liquid state.
Question 5
1 / -0

Which of the following is extensive property?

A
Specific heat capacity

B
Entropy

C
Temperature

D
Refractive index

Solution

Intensive properties: Properties which are independent of the amount of substance (or substances) present in the system are called intensive properties, e.g. pressure, density, temperature, viscosity, surface tension, refractive index, emf, chemical potential, sp. heat etc, These are intensive properties.
So, we can say that entropy is an extensive property.
Question 6
1 / -0

Which of the following is true about a spontaneous process?

A
Spontaneity does not depend on Gibbs energy.

B
Gibbs energy change is less than 0.

C
Gibbs energy change is 0.

D
Gibbs energy change is greater than 0.

Solution

In cases where ΔG is: negative, the process is spontaneous and proceed in the forward direction.
Question 7
1 / -0

For a spontaneous chemical process, the free energy change is

A
not measurable

B
negative

C
positive

D
zero

Solution

The sign of ΔG will change from positive to negative (or vice versa) where T = ΔH/ΔS. In cases where ΔG is: negative, the process is spontaneous and may proceed in the forward direction as written. positive, the process is non-spontaneous as written, but it may proceed spontaneously in the reverse direction.
Question 8
1 / -0

Which of the following statements is correct about the process of evaporation of water from an open beaker?

A
It is a spontaneous and endothermic process.

B
It is a non-spontaneous and endothermic process.

C
It is a spontaneous and exothermic process.

D
It is a non-spontaneous and exothermic process.

Solution

Evaporation of water from an open pot is a spontaneous process. As it starts on its own without any external agent. However it takes heat from surrounding means that it is endothermic.
Question 9
1 / -0

Which of the following is NOT a state function?

A
q + w

B
q

C
q_rev/T

D
PV

Solution

A state function is the property of the system whose value depends only on the initial and final state of the system and is independent of the path. It is a state function because it is independent of the path. Heat (q) and work (W) are not state functions being path dependent.
Question 10
1 / -0

The equilibrium constant for a reaction is 10. Calculate the value of ΔG° at 300K

A
-5.527 kJ/mol^–

B
4.744 kJ/mol

C
-4.744 kJ/mol^–

D
- 5.744 kJ/mol

Solution

The value of equilibrium constant(k) = 10
∆G° = -2.303RTlogk
On calculating values, we will get ∆G° = -5.744kJmol^-1

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Thermodynamics Test - 27

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Thermodynamics Test - 27

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Question 1

does not change

increases

decreases

first increases and then decreases

Solution

Question 2

ΔSTotal is constant

ΔSTotal > 0

ΔSTotal < 0

ΔSTotal = 0

Solution

Question 3

Entropy of water increases.

Entropy of water becomes zero.

Entropy of water decreases.

Entropy of water remains same.

Solution

Question 4

Negative

Positive

Both positive and negative

None of the above

Solution

Question 5

Specific heat capacity

Entropy

Temperature

Refractive index

Solution

Question 6

Spontaneity does not depend on Gibbs energy.

Gibbs energy change is less than 0.

Gibbs energy change is 0.

Gibbs energy change is greater than 0.

Solution

Question 7

not measurable

negative

positive

zero

Solution

Question 8

It is a spontaneous and endothermic process.

It is a non-spontaneous and endothermic process.

It is a spontaneous and exothermic process.

It is a non-spontaneous and exothermic process.

Solution

Question 9

q + w

q

qrev/T

PV

Solution

Question 10

-5.527 kJ/mol–

4.744 kJ/mol

-4.744 kJ/mol–

- 5.744 kJ/mol

Solution

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ΔS_Total is constant

ΔS_Total > 0

ΔS_Total < 0

ΔS_Total = 0

q_rev/T

-5.527 kJ/mol^–

-4.744 kJ/mol^–