exothermicIs the reaction exothermic or endothermic?endothermicupDoes the temperature of the water bath go up ordown?downneitherinDoes the piston move in or out?outneitherinDoes heat flow into or out of the gas mixture?outneitherHow much heat flows? Be sure your answer hasthe correct number of significant digits. A mixture of gaseous reactants is put into a cylinder, where a chemical reaction turns them into gaseous products. Thecylinder has a piston that moves in or out, as necessary, to keep a constant pressure on the mixture of 1 atm. Thecylinder is also submerged in a large insulated water bath. (See sketch at right.)From previous experiments, this chemical reaction is known to release 114. kJ of energy.The position of the piston is monitored, and it is determined from this data that the piston does 370. kJ of work on thesystem during the reaction.

Work is done by the system, sign will be negative. Work is done on the system, sign will be…

exothermic Is the reaction exothermic or endothermic? endothermic up Does the temperature of the water bath go up or down? down neither in Does the piston move in or out? out neither in Does heat flow into or out of the gas mixture? out neither How much heat flows? Be sure your answer has the correct number of significant digits.

exothermic Is the reaction exothermic or endothermic? endothermic up Does the temperature of the water bath go up or down? down neither in Does the piston move in or out? out neither in Does heat flow into or out of the gas mixture? out neither How much heat flows? Be sure your answer has the correct number of significant digits.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 37E: Consider a mixture of air and gasoline vapor in a cylinder with a piston. The original volume is 40....

See similar textbooks

Similar questions

Evaporation of sweat requires energy and thus take excess heat away from the body. Some of the water that you drink may eventually be converted into sweat and evaporate. If you drink a 20-ounce bottle of water that had been in the refrigerator at 3.8 C, how much heat is needed to convert all of that water into sweat and then to vapor? (Note: Your body temperature is 36.6 oc. For the purpose of solving this problem, assume that the thermal properties of sweat are the same as for water.)
he following demonstration takes place in a two-step process: rst, solid calcium carbide (CaC2j)reacts with liquid water to produce acetylene gas (C2H2)and aqueous calcium hydroxide. Second the acetylene gas produced is then ignited with a match, causing the combustion reaction of acetylene with oxygen gas to produce gaseous carbon dioxide and gaseous water. Write the balanced equations for each reaction that is occurring, including all phases. If a 100.0gsample of calcium carbide (CaC2)is initially reacted with 50.0gof water, which reactant is limiting? Now imagine that the final gases produced are collected in a large bulkier and allowed to cool to room temperature. Using the information from part b ( l00.0gof Cec2reacting with 50.0gof H2O), how many liters of carbon dioxide gas were produced in the balloon at a pressure of 1.00atm and 25C?
In regions with dry climates, evaporative coolers are used to cool air. A typical electric air conditioner is rated at 1.00 104 Btu/h (1 Btu, or British thermal unit = amount of energy to raise the temperature of 1 lb water by 1F). What quantity of water must be evaporated each hour to dissipate as much heat as a typical electric air conditioner?
Consider a mixture of air and gasoline vapor in a cylinder with a piston. The original volume is 40. cm3. If the combustion of this mixture releases 950. J of energy, to what volume will the gases expand against a constant pressure of 650. torr if all the energy of combustion is converted into work to push back the piston?
97 Homes in rural areas where natural gas service is not available often rely on propane to fuel kitchen ranges. The propane is stored as a liquid, and the gas to be burned is produced as the liquid evaporates. Suppose an architect has hired you to consult on the choice of a propane tank for such a new home. The propane gas consumed in 1.0 hour by a typical range burner at high power would occupy roughly 165 L at 25°C and 1.0 atm, and the range chosen by the client will have six burners. If the tank under consideration holds 500.0 gallons of liquid propane, what is the minimum number of hours it would take for the range to consume an entire tankful of propane? The density of liquid propane is 0.5077 kg/L.
A sample of steam with a mass of 0.521 g at a temperature of 100 oC condenses into an insulated container holding 4.50 g of water at 5.0 .C. For water, \Delta Hovap = 40.7 kJ/mol and Cwater = 4.18 J/(g-oC). Part A Assuming that no heat is lost to the surroundings, what is the final temperature of the mixture? Express your answer in degrees Celsius to three significant figures.
Incandescent light bulbs can get very hot to the touch as they convert much of the electrical energy flowing through them into heat. A 60 W light bulb has a volume of 180.0 mL at SATP. The light bulb is switched on and the heated glass expands slightly to 180.5 mL with an internal pressure of 114.5 kPa. The new temperature of the light bulb in degrees C is:
How many joules of work must be done to inflate a balloon to a volume of 3.3 L if atmospheric pressure is 0.44 atm?
9.41 mol of argon gas is admitted to an evacuated 9,472.23 cm3 container at 46.51oC. The gas then undergoes an isochoric heating to a temperature of 242.1oC. What is the final pressure?
The smell of rotten eggs comes from dihydrogen monosulfide, which is created through anaerobic respiration of bacteria in low-oxygen environments. In the lab, however, it can be synthesized by reacting aluminum sulfide with water, with aluminum hydroxide as a byproduct. A chemist synthesizes dihydrogen monosulfide and collects 37.8 mL over water at 298 K and 762 mmHg. Assuming water was the excess reactant, what mass of aluminum sulfide was reacted?
this is at constant pressure. object expands another object to initial volume of 75 m^3 to final volume of 100 m^3. object released 170 kJ of heat into gas during and change in internal energy is -180 kJ... what is pressure in kPA of gas in the container
Suppose you are overtaken by a blizzard while ski touring and you take refuge in a tent. You arethirsty, but you forgot to bring liquid water. You have a choice of eating a few handfuls of snow (say400 g) at −5.0 °C immediately to quench your thirst or setting up your propane stove, melting thesnow, and heating the water to body temperature before drinking it. You recall that the survival guide you leafed through at the hotel said something about not eating snow, but you cannotremember why–after all, it’s just frozen water. To understand the guide’s recommendation, calculatethe amount of heat that your body will have to supply to bring 400. g of snow at −5.0 °C to yourbody’s internal temperature of 37 °C. The specific heats of liquid water and ice are 4.184 J/(g•°C) and2.062 J/(g•°C), respectively, and the enthalpy of fusion of ice is 6.01 kJ/mol.

Recommended textbooks for you

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781133949640

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry