Chapter 3Question 1:Convert the following energy units. a) 5.60 × 102 kJ to Jb) 2850 kcal to kJc) 5.85 × 106 J to kcalQuestion 2:At constant pressure, which of these systems do work on the surroundings? Check all thatapply.2A(g) + B(g) → C(g) A(g) + B(g) → 3C(g) A(s) + B(g) → 2C(g) A(g) + B(g) → C(g)Question 3:How much work must be done on a system to decrease its volume from 11.0 L to 4.0 L by exerting a constant pressure of 4.0 atm?Question 4:Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 10.0 atm.Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 15.0 L.Now calculate the work done if this process is carried out in two steps. 1. First, let the gasexpand against a constant external pressure of 5.00 atm to a volume of 3.00 L. 2. From there, let the gas expand to 15.0 L against a constant external pressure of 1.00 atm.Question 5:If a system has 275 kcal of work done to it, and releases 5.00 × 102 kJ of heat into its surroundings, what is the change in internal energy of the system?Question 6:Classify each of the following as a path function or a state function: heat, energy, enthalpy, work, distance traveled.Question 7:The specific heat of a certain type of cooking oil is 1.75 J/(g·°C). How much heat energy is needed to raise the temperature of 2.03 kg of this oil from 23 °C to 191 °C?Question 8:A 57.89 g sample of a substance is initially at 28.4 °C. After absorbing 1769 J of heat, thetemperature of the substance is 173.0 °C. What is the specific heat (c) of the substance?Question 9:The specific heat of a certain type of metal is 0.128 J/(g·°C). What is the final temperature if 305 J of heat is added to 89.1 g of this metal initially at 20.0 °C?Question 10:An 80.0-gram sample of a gas was heated from 25 °C to 225 °C. During this process, 346J of work was done by the system and its internal energy increased by 8795 J. What is the specific heat of the gas?Question 11:When 1752 J of heat energy is added to 37.4 g of ethanol, C2H6O, the temperature increases by 19.1 °C. Calculate the molar heat capacity of C2H6O.Question 12:Consider the following reaction.Theformation of 75.0 g of Fe results in:the release of 15500 kJ of heatthe absorption of 1110 kJ of heatthe absorption of 15500 kJ of heatthe absorption of 277 kJ of heatthe release of 277 kJ of heatthe release of 1110 kJ of heatQuestion 13:Using the standard enthalpies of formation, what is the standard enthalpy of reaction?Question 14:Given thatcalculate the value of ΔH°rxn forQuestion 15:The 1995 Nobel Prize in Chemistry was shared by Paul Crutzen, F. Sherwood Rowland, and Mario Molina for their work concerning the formation and decomposition of ozone in thestratosphere. Rowland and Molina hypothesized that chlorofluorocarbons (CFCs) in the stratosphere break down upon exposure to UV radiation, producing chlorine atoms. Chlorine waspreviously identified as a catalyst in the breakdown of ozone into oxygen gas. Using the enthalpy of reaction for two reactions with ozone, determine the enthalpy of reaction for the reaction of chlorine with ozone.Question 16:Use the molar bond enthalpy data in the table to estimate the value of ΔH°rxn for the equationThe bonding in the molecules is shown here.Question 17:SkippedQuestion 18:When a 4.00-g sample of RbBr is dissolved in water in a calorimeter that has a total heat capacity of 1.471 kJ·K–1, the temperature decreases by 0.360 K. Calculate the molar heat of solution of RbBr.Question 19:In a constant-pressure calorimeter, 50.0 mL of 0.310 M Ba(OH)2 was added to 50.0 mL of 0.620 M HCl. The reaction caused the temperature of the solution to rise from 24.02 °C to 28.24 °C. If the solution has the same density and specific heat as water, what is ΔH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes.Question 20:When methanol, CH3OH, is burned in the presence of oxygen gas, O2, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the following balanced, thermochemical equation:How much methanol (in grams) must be burned to produce 753 kJ of