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
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