Five moles of monatomic ideal gas enter the abc cycle and during a complete cycle 600 J of heat is removed from the gas. Process ab is under constant pressure and process bc is increasing at constant volume takes place at pressure. The temperatures of points a and b are Ta= 3°C and Tb= 63°C. What is the work in the ca process?

Five moles of monatomic ideal gas enter the abc cycle and during a complete cycle 600 J of heat is removed from the gas. Process ab is under constant pressure and process bc is increasing at constant volume takes place at pressure. The temperatures of points a and b are Ta= 3°C and Tb= 63°C. What is the work in the ca process?

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A 6.91 mol sample of ethylene is burned in a bomb calorimeter that has heat capacity of 348.0 J°C^-1. The temperature of the water jacket rises from 24.83°C to 31.92°C. Calculate Delta E for the combustion of one mole of ethylene.
A refrigerator works by forcing heat out of the system and reverses the direction of the Carnot cycle. If a refrigerator containing 1.00 mole of gas has an initial temperature of 298 K, what is the total amount of work it would require to cool the refrigerator to 273 K.? What is the maximum efficiency of this process? Assume CV= 3R/2, VA= 2.00 L, VB= 10.0 L, VC= 11.4 L, and VD= 2.28 L.
Suppose dilute hydrochloric acid is poured on to some calcium carbonate in an open vessel and 1.0 mol CO2(g) is produced at 25 °c. How much expansion work is done?
5b.
A geochemist in the field takes a 47.0 mL sample of water from a rock pool lined with crystals of a certain mineral compound X. He notes the temperature of the pool, 17.° C, and caps the sample carefully.. Back in the lab, the geochemist filters the sample and then evaporates all the water under vacuum. Crystals of X are left behind. The researcher washes, dries and weighs the crystals. They weigh 8.93 g. |yes Using only the information above, can you calculate olo the solubility of X in water at 17.° C? no Ar If you said yes, calculate it. Be sure your answer has a unit symbol and the right number of significant digits.
A solution of 75.0 mL of 3.20 M HNO3 was mixed with 50.0 mL of 2.00 M Ca(OH)2 in a large Styrofoam coffee cup; the cup is fitted with a lid through which a calibrated thermometer passes. The temperature of both solutions before mixing was 20.1 °C. After the Ca(OH)2 solution is added to the coffee cup and the mixed solutions are stirred with the thermometer, the maximum temperature measured was 39.2 °C. Assume that the volumes are additive but that the density of the mixed solution is 1.10 g/mL, the specific heat of the mixed solution is 4.18 J/g•°C, and no heat is lost to the surroundings. In much the same way as you did for the previous question, calculate the enthalpy change per mole of HNO3 in the reaction. Consider that only reactants that actually react will account for the heat produced.
(2B) A heat engine operates between a hot source at 130.°C and a cold sink at 10.°C. How much workcan be done by the engine if 523 kJ of heat are extracted from the hot source?
please solve this quickly
A 110.2 mL sample of 1.00 M NaOH is mixed with 55.1 mL of 1.00 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 21.85 °C. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 31.30 °C. Assume that the density of the mixed solutions is 1.00 g/mL, that the specific heat of the mixed solutions is 4.18 J/(g·°C), and that no heat is lost to the surroundings. a. Write a balanced chemical equation for the reaction that takes place in the Styrofoam cup. Remember to include phases in the balanced chemical equation. b. Is any NaOH or H2SO4 left in the Styrofoam cup when the reaction is over?A. No B. Yes c. Calculate the enthalpy change per mole of H2SO4 in the reaction. kJ/mol
The internal pressure of a gas, π = au dv)T' is a measure of intermolecular forces, because it indicates a change in internal energy as the molecules get closer or further apart, without temperature changing. = a Calculate the change in internal 1 Vm T energy, AU, when 1.5 mols of acetone (a = 16 l² atm/mo1²), expands from 2 liters to 5 liters at a constant temperature. ii) Would this change in internal energy be greater or smaller for an ideal gas? Why? i) Using the van der Waals equation of state, T = au
If 54.0 g argon at 400 K is compressed isothermally and reversibly from a pressure of 1.50 to 4.00 atm, calculate the work done on the gas and the heat absorbed by gas in the process. What are the changes in energy (AU) and in enthalpy (AH) of the gas?
4.00 g NaOH(s) (39.996 g mol–1) dissolves in 100.0 g of water in a constant–pressure calorimeter. The initial temperatures of both materials are the same at 20.0°C. The density of the solution is 1.00 g cm–3. The heat of dissolution is –44.51 kJ mol–1. The specific heat of the solution is 4.184 J g–1 °C–1. The specific heat of the calorimeter is 100 J °C–1. What is the final temperature of the solution? 30.23°C 25.94°C 28.32°C What is the energy lost to the calorimeter? 579 J 832 J 721 J