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?

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 67AP

See similar textbooks

Similar questions

The following are values of heat capacity for nitrogen gas; Temp K Cv J/mol. K 300 20.8 400 20.9 500 21.2 600 21.8 700 22.4 800 23.1 900 23.7 1000 24.3 1100 24.9 Using the general formula Cv = A BT C/T2, find values of A, B, and C that fit the given data.
Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.
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!)
Use the data in Table 2.2 to determine Hp T for Ar at 0C and 1atm. Make any reasonable assumptions necessary.
Use the two appropriate values of R to determine a conversion between L. atm and J.
What is the finaltemperature of0.122 mole ofmonatomic ideal gas that performs 75J of work adiabatically if the initial temperature is 235C?
Limestone stalactites and stalagmites are formed in caves by the following reaction:Ca2+(aq)+2HCO−3(aq)→CaCO3(s)+CO2(g)+H2O(l)Ca2+(aq)+2HCO3−(aq)→CaCO3(s)+CO2(g)+H2O(l)If 1 molmol of CaCO3CaCO3 forms at 298 KK under 1 atmatm pressure, the reaction performs 2.47 kJkJ of P−VP−V work, pushing back the atmosphere as the gaseous CO2CO2 forms. At the same time, 38.75 kJkJ of heat is absorbed from the environment. What is the value of ΔHΔH for this reaction? Express your answer using four significant figures.
a sample of 98g of pure sulfuric acid is dissolved in 2.0 kg of water in an insulated vessel at 15°C, and thetemperature rises rapidly because of the process of forming the solution. The reaction is summarized in theequation H2SO4(l) -> H+(aq) + HSO4 –(aq). Estimate the temperature change assuming that the heat capacityof the solution is 4.0 J/gK and the heat capacity of the vessel is 300 J/K.
A 1.65 mole sample of an ideal gas for which Cv, m = 3/2 R undergoes the following two-step process: (a) From an initial state of the gas described by T = 14.5 oC and P = 2x104 Pa, the gas undergoes isothermal expansion against a constant external pressure of 1.0x104 Pa until the volume has doubled. (b) Then the gas is cooled to constant volume. The temperature drops to -35.6 oC. Calculate q, w, ΔH, ΔU for each step and for the overall process.
a) A 1.60 dm3 sample of a mixture of methane gas, CH4 and oxygen gas, measured at 25 oC and 101 kPa, was allowed to react in a bomb calorimeter in which, had a heat capacity of 5.30 kJ/K altogether with its contents. The complete combustion of the methane gas to carbon dioxide gas and water caused a temperature rise in the calorimeter of 6.28 K. Given that ∆Ho c (CH4) is -560 kJ/mol. i. Define the standard enthalpy of combustion of methane ii. Write a thermochemical equation for the combustion of methane iii. Knowing the ∆Ho c of methane, calculate the number of mole of methane in the mixture. iv. Calculate the total moles of gases in the calorimeter.
Chemistry Work is done in this reaction when the H2 gas expands out of the test tube and pushes the atmosphere aside. W = PV where W = work, P = pressure, V = Vfinal - Vinitial work done with one mole of Mg reacts with excess acid at STP= 314.1J Q1: Assuming the same amount of Mg reacted, which value should be larger - the heat measured under constant pressure conditions or the heat measured under constant volume conditions? Explain. Q 2: The literature value for the heat produced when Mg reacts with H+ under constant pressure conditions is - 110 kcal/mol. Calculate the accuracy obtained from this experiment.