CHM1100C Module 06 Quiz Latest 2023

CHM1100C Section 06 General Chemistry

Module 06 Quiz

Question 1

What is the difference between the heat capacity and specific heat of a substance?

Question 2

Describe the difference between an exothermic and endothermic process in terms of a chemical compound or reaction.

Question 3

How does Gibbs energy, enthalpy, and entropy determine whether a process will be a spontaneous or nonspontaneous reaction?”

Question 4

Explain the difference between the 3 energy systems and provide a real-world example of a system of energy.

Question 5

Describe the differences between the first, second and third law of thermodynamics.

Question 6

If the energy of the system is the sum of the energy and work, identify the following: What would be the sign of energy (Q) if the system was releasing heat?

Question 7

If the energy of the system is the sum of the energy and work, identify the following: What would be the sign of energy (Q) if the system was absorbing heat?

Question 8

Solve the following thermochemical reactions:

2 HCl + Pb

PbCl2+ H2

H = -1861 J/mole

What is the enthalpy if there was 4.5 x 10-3g of HCl?

Question 9

Solve the following thermochemical reactions:

2 HCl + Pb

PbCl2 + H2

H = -1861 J/mole

What is the enthalpy if there was 3.86g of PbCl2?

Question 10

Calculate the amount of heat absorbed or released by the following substances: 65.3g of nitrogen,

T = 334K

 Question 11

Calculate the amount of heat absorbed or released by the following substances: 34.6g of water, final temperature = 60°C, initial temperature = 44°C

Question 12

Describe if the following reaction is spontaneous or non-spontaneous based on enthalpy, entropy and Gibbs energy:

H = -7458J/mol,

S = -3756J/K*mol, and

G = -436J at low temperature

Question 13

Describe if the following reaction is spontaneous or non-spontaneous based on enthalpy, entropy and Gibbs energy:

H = 8457J/mol,

S = 546J/K*mol, and

G = 432J at room temperature

Question 14

Predict the trend of entropy in the following scenario: Freezing of water

Question 15

Predict the trend of entropy in the following scenario: Salt dissolving in water

Question 16

Predict the trend of entropy in the following scenario: Entropy of helium v. entropy of Argon

Hide answer choices

1.Entropy is higher

2.Entropy is lower

3.No change in entropy

Question 17

Predict the trend of entropy in the following scenario: Water as steam compared to liquid

Question 18

Calculate the reaction entropy ( S°rxn) for the following reaction: 2 LiOH + CO2  Li2CO3 + H2O

Question 19

Calculate the reaction entropy ( S°rxn) for the following reaction: HCl + NaOH NaCl + H2O

Question 20

Calculate the Gibbs energy for the following condition K = 8.2 x 10-11, T = 35?C

Question 21

What is the heat required for a substance that has a mass of 633g, specific heat of 2.454J/g C to change from room temperature to 45C?

Question 22

Write out the equilibrium constant expressions for the following reaction: 2 KClO3 (s) → 2 KCl (s) + 3 O2 (g)

Question 23

Write out the equilibrium constant expressions for the following reaction: H2O (l) → H+ (aq) + OH- (aq)

Question 24

Consider an exothermic reaction. How does the following action affect an equilibrium reaction by driving the reaction? Increasing the temperature of the system

1.Forward reaction

2.Reverse reaction

Question 25

Consider the endothermic reaction N2(g) + 3H2(g) ? 2NH3(g). How does the following action affect an equilibrium reaction by driving the reaction? Decreasing volume of the system, while increasing the pressure

1.Forward reaction

2. Reverse reaction