An idenl diatomic gas has a molar internal energy equal to E =RT which depends only on its absolute temperature T. A mole of this gas is taken quasi- statically first from state A to state B, and then from state B to state C along the straight line paths shown in the diagram of pressure p versus volume V. (a) What is the molar heat capacity at constant volume of this gas? (b) What is the work done by the gas in the process A → B→ C? (c) What is the heat absorbed by the gas in this process? (d) What is its change of entropy in this process? B 8 2 1 2 3 (10' cm

An idenl diatomic gas has a molar internal energy equal to E =RT which depends only on its absolute temperature T. A mole of this gas is taken quasi- statically first from state A to state B, and then from state B to state C along the straight line paths shown in the diagram of pressure p versus volume V. (a) What is the molar heat capacity at constant volume of this gas? (b) What is the work done by the gas in the process A → B→ C? (c) What is the heat absorbed by the gas in this process? (d) What is its change of entropy in this process? B 8 2 1 2 3 (10' cm

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 58P

See similar textbooks

Similar questions

Many compressed gases come in large,heavy metal cylindersthat are so heavy that they need a special cart to move them around. An80.0-Ltank ofnitrogen gas pressurized to 172 atm is left in the sun and heats from its normal temperature of 20.0C to 140.0C. Determine a the final pressureinsidethe tank and b the work, heat, and U of the process. Assume that behavior is ideal and the heatcapacity of diatomic nitrogenis 21.0J/mol.K.
What are the numerical values of the heat capacities c-v and c-p of a monatomic ideal gas,in units of cal/mol.K and L.atm/mol.K?
What is the finaltemperature of0.122 mole ofmonatomic ideal gas that performs 75J of work adiabatically if the initial temperature is 235C?
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.
Show that = T/p for an ideal gas.
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!)
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.
Estimate the contribution of motion to the molar internal energyof nitrogen gas.
The n-butane is converted into isobutane in an isomerization reactor, which operates isothermally at 149°C. Suppose that the reactor is fed with a mixture containing 93% mole of n-butane, 5% isobutane and 2% HCl at 149°C and that a 40% conversion of n-butane is achieved. How much heat in KJ/m3 (STP) of the feed, should be supplied or extracted from the reactor?
o-phthalic acid, C8H6O4, is sometimes used as a calorimetric standard. Its heat ofcombustion is - 3.224 × 103 kJ/mol C8H6O4. From the following data determine theheat capacity of a bomb calorimeter assembly (i.e., of the bomb, water, stirrer,thermometer, wires, etc.)mass of o-phthalic acid burned: 1.078 ginitial calorimeter temperature 24.96 °Cfinal calorimeter temperature 30.76 °C
What is the standard enthalpy of formation of the decomposition of one mole of liquid sulfuric acid to steam, oxygen, and sulfur dioxide gas?
A sample of pure solid naphthalene (C10H8) weighing 0.6410 g is burned completely with oxygen to CO2(g) and H2O(,) in a constant-volume calorimeter at 25°C. The amount of heat evolved is observed to be 25.79 kJ. (a) Write and balance the chemical equation for the combustion reaction. (b) Calculate the standard change in internal energy (DU°) for the combustion of 1.000 mol naphthalene to CO2(g) and H2O(,). (c) Calculate the standard enthalpy change (DH°) for the same reaction as in part (b). (d) Calculate the standard enthalpy of formation per mole of naphthalene, using data for the standard enthalpies of formation of CO2(g) and H2O(,) from Appendix D.