End of Module 16 Quiz

Based on first law of thermodynamics

As per the second Law of thermodynamics

Which of the following statements are true?

Entropy is the measure of

As per the third law of thermodynamics

Find the boiling point of compound A, based on the data for the reaction shown below.

A (l) A (g), Given ∆S = 165 J/mol, ∆H = 75 KJ/mol K

Using the thermodynamic data given, find the change in entropy for the following reaction.
∆S N 2 (g) = 191.5 J/mol. K, ∆S H 2 = 130.6 J/mol.K, ∆S NH 3 (g) = 192.3 J/mol.K
N 2 (g) + 3H 2 (g) 2NH 3 (g)

Using the thermodynamic data given, find the change in entropy for the surrounding for the
following reaction at 25 °C.

∆H N 2 (g) = 0 KJ/mol, ∆H H 2 = 0 KJ/mol, ∆H NH 3 (g) = -46.1 KJ/mol
N 2 (g) + 3H 2 (g) 2NH 3 (g)

Using the thermodynamic data given, find the change in entropy for the universe for the
following reaction.
∆S system = – 199.0 J/mol. K, ∆S surrounding = 309 J/mol. K
N 2 (g) + 3H 2 (g) 2NH 3 (g)

Using the thermodynamic data given, find the change in Gibbs free energy for the following
reaction.
∆G P(s) = 10.0 kj/mol, ∆G H 2 = 0 kj/mol, ∆G PH 3 (g) = 25.5 Kj/mol
2P (s) + 3H 2 (g) 2PH 3 (g)

If ∆G° for a reaction is -25.5 KJ, will the reaction be spontaneous under the same conditions of
temperature and pressure?

Calculate ∆G for the following reaction A + B C + D, based on thermodynamic data
collected at 25 °C. ∆ S = -85.5 J and ∆H = -65.8 KJ

Looking at the reaction below, what can you predict about the spontaneity of the reaction
(Hint: look at the sign of ∆H and ∆S to decide the sign of ∆G)
CO 2 (s) CO 2 (g)

Looking at the reaction below, what can you predict about the spontaneity of the reaction
(Hint: look at the sign of ∆H and ∆S to decide the sign of ∆G)
2H 2 (g) + O 2 (g) 2H 2 O (l) ∆H = -570 kj/mol

Looking at the reaction below, what can you predict about the spontaneity of the reaction
(Hint: look at the sign of ∆H and ∆S to decide the sign of ∆G)
A 2 (g) + B 2 (g) 2AB(s) ∆H = 570 kj/mol

Find the equilibrium constant for the reaction given below at 25 °C.
2NH 3 (g) N 2 (g) + 3H 2 (g) ∆G° = 33 kj/mol of N 2

Find the ∆G for the reaction given below at 25 °C under non standard conditions. Partial
pressure of each gas is given below.
2NH 3 (g) N 2 (g) + 3H 2 (g) ∆G = 33 kj/mol of N 2
P(NH 3 ) = 15.5 atm, P(N 2 ) = 0.75 atm and P(H 2 ) = 0.015 atm

Based on thermodynamic data given, find the Ksp for the reaction at 25 °C.
CaCO 3 Ca +2 + CO 3 -2
(∆G° Ca +2 =-553 kj/mol , ∆G° CO 3 -2 = -528 kj/mol , ∆G° CaCO 3 = -1129 KJ/mol)

Which of the following is true for a reaction at equilibrium?

A reaction has a negative Gibbs free energy value. Which of the following statements is true?

Which of the following represents the relation between Gibbs free energy, enthalpy and entropy
change for a reaction?

Which of the following is the measure of randomness?

Which of the following will have highest entropy?

Which of the following processes will result in decrease in entropy?

Which of the following reactions will result in decrease in entropy?

Which of the following processes will result in a decrease in entropy?

Which of the following processes will result in an increase in entropy?