14. Which of the following statements are true about a system that absorbs 300J of heat from thesurroundings while performing 150 J of work on the surroundings?I.The internal energy change of the system is +150 J.The process described above is exothermic.The internal energy change of the system is -150 J.The process described above is endothermic.II.III.IV.а. I, IIb. II, IIIс. I, IVd. III, IV

Heat (q) is positive if heat is added to the system, and negative if heat is removed.Work (W) is…

Answered: 14. Which of the following statements…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 14P

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In earlier times, ethyl ether was commonly used as an anesthetic. It is, however, highly flammable. When five milliliters of ethyl ether, C4H10O(l)(d=0.714g/mL), are burned in a bomb calorimeter, the temperature rises from 23.5C to 39.7C. The calorimeter contains 1.200 kg of water and has a heat capacity of 5.32 kJ/C. (a) What is qH2o? (b) What is qcal? (c) What is q for the combustion of 5.00 mL of ethyl ether? (d) What is q for the combustion of one mole of ethyl ether?
Dry ice is solid carbon dioxide; it vaporizes at room temperature and normal pressures to the gas. Suppose you put 21.5 g of dry ice in a vessel fitted with a piston (similar to the one in Figure 6.9 but with the weight replaced by the atmosphere), and it vaporizes completely to the gas, pushing the piston upward until its pressure and temperature equal those of the surrounding atmosphere at 24.0C and 751 mmHg. Calculate the work done by the gas in expanding against the atmosphere. Neglect the volume of the solid carbon dioxide, which is very small in comparison to the volume of the gas phase.
9.42 Why is enthalpy generally more useful than internal energy in the thermodynamics of real world systems?
Aballoon filled with 0.505 mole of gascontracts reversibly from 1.0L to 0.10 L ata constant temperature of 5.0C. In doing so, it loses 2690J of heat. Calculate w, q, U, and H for the process.
As a gas cools, it is compressed from 2.50 L to 1.25 L under a constant pressure of 1.01 105 Pa. Calculate the work (in J) required to compress the gas.
In which of the following systems is(are) work done by the surroundings on the system? Assume pressure and temperature are constant. a. 2SO2(g)+O2(g)2SO3(g) b.CO2(s)CO2(g) c. 4NH3(g)+7O2(g)4NO2(g)+6H2O(g) d.N2O4(g)2NO2(g) e.CaCO3(s)CaCO(s)+CO2(g)
When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and CO2(g) are formed with the evolution of 19.18 kJ of heat. a Calculate the molar enthalpy of formation of ethylene glycol. (It will be necessary to use data from Appendix C.) b Gf of ethylene glycol is 322.5 kJ/mol. What is G for the combustion of 1 mol ethylene glycol? c What is S for the combustion of 1 mol ethylene glycol?
Consider the reaction 2HCl(aq)+Ba(OH)2(aq)BaCl2(aq)+2H2O(l)H=118KJ Calculate the heat when 100.0 rnL of 0.500 M HCl is mixed with 300.0 mL of 0.100 M Ba(OH)2 Assuming that the temperature of both solutions was initially 25.0C and that the final mixture has a mass of 400.0 g and a specific heat capacity of 4.18 J/C g, calculate the final temperature of the mixture.
9.100 Two baking sheets are made of different metals. You purchase both and bake a dozen cookies on each sheet at the same time in your oven. You observe that after 9 minutes, the cookies on one sheet are slightly burned on the bottom, whereas those on the other sheet are fine. (You are curious and you vary the conditions so you know the result is not caused by the oven.) (a) How can you use this observation to infer something about the specific heat of the materials in the baking sheets? (b) What is themathematical reasoning (equation) that you need to support your conclusion?
A balloon expands from 0.75 L to 1.20 L as it is heated under a constant pressure of 1.01 105 Pa. Calculate the work (in J) done by the balloon on the environment.
When 1.000 g of gaseous butane, C4H10, is burned at 25C and 1.00 atm pressure, H2O(l) and CO2(g) are formed with the evolution of 49.50 kJ of heat. a Calculate the molar enthalpy of formation of butane. (Use enthalpy of formation data for H2O and CO2.) b Gf of butane is 17.2 kJ/mol. What is G for the combustion of 1 mol butane? c From a and b, calculate S for the combustion of 1 mol butane.

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