6. An air conditioner takes outside air at 35°C and cools it to 15 °C at a rate of 1 kg/s. Estimate theamount of power needed to do this for a Carnot cycle. Consider air an ideal gas with a constantheat capacity (15 pt)Note. A refrigerant is the working fluid for an air conditioner.Inside airTLEvaporator43ExpansionvalveCompressorW2An air conditioner in cooling modeOutside airCondenserΤΗ

Answered: 6. An air conditioner takes outside air…

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.32E: Many compressed gases come in large,heavy metal cylindersthat are so heavy that they need a special...

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Similar questions

The Dieterici equation of state for one mole of gas is p=RTe-aVRTV-b Where a and b are constants determined experimentally. For NH3g, a = 10.91 atm. L2 and b = 0.0401 L. Plot the pressure of the gas as the volume of 1.00 mol of NH3g expands from 22.4 L to 50.0 L at 273 K, and numerically determine the work done by the gas by measuring the area under the curve.
A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it exerts pressure of 2000 psi. Calculate the work (in J) performed when this gas expands isothermally against an opposing pressure of 1.0 atm. (The amount of work that can be done is equivalent to the destructive force of about 1/4 lb of dynamite, giving you an idea of how potentially destructive compressed gas cylinders can be if improperly handled!)
The enthalpy of vaporization for water is 40.65 kJ mol-1. As a design engineer for a project in a desert climate, you are exploring the option of using evaporative cooling. (a) If the air has an average volumetric heat capacity of 0.00130 J cm-3 K-1, what is the minimum mass of water that would need to evaporate in order to cool a 5 m? 5 m room with a 3 m ceiling by 5°F using this method? (b) Is this a spontaneous or nonspontaneous process?
Explain why the high-temperature reservoir of a heat engine must, indeed, be higher in temperature than the low-temperature reservoir. Can it ever be the other way around?
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?
Use the data in Table 2.2 to determine Hp T for Ar at 0C and 1atm. Make any reasonable assumptions necessary.
9.11 Analyze the units of the quantity (pressurevolume) and show that they are energy units, consistent with the idea of PV-work.
In thermodynamics, the pathway in a pressure-volume diagram for an adiabatic change is called an adiabat, while the pathway for an isothermal change is called an isotherm. Identify the adiabats and isotherms in Figure 3.2.
Nitromethane, CH3NO2, is a good fuel. It is a liquid at ordinary temperatures. When the liquid is burned, the reaction involved is chiefly 2CH3NO2(l)+32O2(g)2CO2(g)+N2(g)+3H2O(g) The standard enthalpy of formation of liquid nitromethaneat 25°C is 112kJmol1; other relevant values can be found in Appendix D. Calculate the enthalpy change in the burning of 1 molliquid nitromethane to form gaseous products at25°C. State explicitly whether the reaction is endothermicor exothermic. Would more or less heat be evolved if gaseous nitromethanewere burned under the same conditions?Indicate what additional information (if any) you would need to calculate the exact amount of heat, and show just how you would use this information.
How many moles of isooctane must be burned to produce loo U of heat under standard state conditions?
What are the two ways that a final chemical state of a system can be more probable than its initial state?
Calculate rS for each substance when the quantity of thermal energy indicated is transferred reversibly to the system at the temperature specified. Assume that youhave enough of each substance so that its temperatureremains constant as the thermal energy is transferred. (a) H2(g), 0.775 kJ/mol, 295 K (b) KCl(s), 500. kJ/mol, 500. K (c) N2(g), 2.45 kJ/mol, 1000. K

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