Homework 3.docxVIP

Chapter 51.(a) Why is the change in enthalpy usually easier to measurethan the change in internal energy? (b) H is a state function,but q is not a state function. Explain. (c) For a given process atconstant pressure, ΔH is positive. Is the process endothermicor exothermic?2.3.4.(a)What are the units of molar heat capacity? (b)What are theunits of specific heat? (c) If you know the specific heat of copper,what additional information do you need to calculate theheat capacity of a particular piece of copper pipe?5.(a) What is the specific heat of liquid water? (b) What is themolar heat capacity of liquid water? (c) What is the heat capacityof 185 g of liquid water? (d) How many kJ of heat areneeded to raise the temperature of 10.00 kg of liquid waterfrom 24.6 °C to 46.2 °C?6.7.Under constant-volume conditions, the heat of combustion ofglucose (C6H12O6) is 15.57 kJ/g. A 3.500-g sample of glucoseis burned in a bomb calorimeter. The temperature of thecalorimeter increased from 20.94 °C to 24.72 °C. (a) What isthe total heat capacity of the calorimeter? (b) If the size of theglucose sample had been exactly twice as large, what would thetemperature change of the calorimeter have been?8.9.10.For each of the following compounds, write a balanced thermochemicalequation depicting the formation of one mole ofthe compound from its elements in their standard states anduse Appendix C to obtain the value of ΔHf°: (a) NO2(g), (b)SO3(g), (c) NaBr(s), (d) Pb(NO3)2(s).11.12.13.14.15.16.17.18.Chapter 101.Imagine that the reaction2 CO(g) + O2(g)2 CO2(g)occurs in a container that has a piston that moves to maintaina constant pressure when the reaction occurs at constant temperature. (a)What happens to the volume of the container as aresult of the reaction? Explain. (b) If the piston is not allowedto move, what happens to the pressure as a result of the reaction?2.(a) How high in meters must a column of water be to exert apressure equal to that of a 760-mm column of mercury? Thedensity of w