CHM1100C Section 06 General ChemistryModule 06 QuizQuestion 1What is the difference between the heat capacity and specific heat of a substance?Question 2Describe the difference between an exothermic and endothermic process in terms of a chemical compound or reaction.Question 3How does Gibbs energy, enthalpy, and entropy determine whether a process will be a spontaneous or nonspontaneous reaction?”Question 4Explain the difference between the 3 energy systems and provide a real-world example of a system of energy.Question 5Describe the differences between the first, second and third law of thermodynamics.Question 6If 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 7If 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 8Solve the following thermochemical reactions:2 HCl + PbPbCl2+ H2H = -1861 J/moleWhat is the enthalpy if there was 4.5 x 10-3g of HCl?Question 9Solve the following thermochemical reactions:2 HCl + PbPbCl2 + H2H = -1861 J/moleWhat is the enthalpy if there was 3.86g of PbCl2?Question 10Calculate the amount of heat absorbed or released by the following substances: 65.3g of nitrogen,T = 334KQuestion 11Calculate the amount of heat absorbed or released by the following substances: 34.6g of water, final temperature = 60°C, initial temperature = 44°CQuestion 12Describe if the following reaction is spontaneous or non-spontaneous based on enthalpy, entropy and Gibbs energy:H = -7458J/mol,S = -3756J/K*mol, andG = -436J at low temperatureQuestion 13Describe if the following reaction is spontaneous or non-spontaneous based on enthalpy, entropy and Gibbs energy:H = 8457J/mol,S = 546J/K*mol, andG = 432J at room temperatureQuestion 14Predict the trend of entropy in the following scenario: Freezing of waterQuestion 15Predict the trend of entropy in the following scenario: Salt dissolving in waterQuestion 16Predict the trend of entropy in the following scenario: Entropy of helium v. entropy of ArgonHide answer choices1.Entropy is higher2.Entropy is lower3.No change in entropyQuestion 17Predict the trend of entropy in the following scenario: Water as steam compared to liquidQuestion 18Calculate the reaction entropy ( S°rxn) for the following reaction: 2 LiOH + CO2 Li2CO3 + H2OQuestion 19Calculate the reaction entropy ( S°rxn) for the following reaction: HCl + NaOH NaCl + H2OQuestion 20Calculate the Gibbs energy for the following condition K = 8.2 x 10-11, T = 35?CQuestion 21What 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 22Write out the equilibrium constant expressions for the following reaction: 2 KClO3 (s) → 2 KCl (s) + 3 O2 (g)Question 23Write out the equilibrium constant expressions for the following reaction: H2O (l) → H+ (aq) + OH- (aq)Question 24Consider an exothermic reaction. How does the following action affect an equilibrium reaction by driving the reaction? Increasing the temperature of the system1.Forward reaction2.Reverse reactionQuestion 25Consider 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 pressure1.Forward reaction2. Reverse reaction
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