Consider a reversible adiabatic expansion of 1.00 mol of an ideal gas, starting from 1.90 L...
Consider a reversible adiabatic expansion of 1.00 mol of an
ideal gas, starting from 1.90 L and 415 K , if 2.0 kJ of work is
done by the expansion. The molar heat capacity at constant volume
of the gas is 2.5R.
R = 8.314 JK−1mol−1.
Determine the final temperature of the gas in the process.
Determine the final volume of the gas in the process.
Determine the final pressure of the gas in the process.
Homework Answers
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Consider a reversible adiabatic expansion of 1.00 mol of an
ideal gas, starting from 1.90 L...
(b) Consider an adiabatic, reversible expansion of 0 020 mol Ar (perfect gas), initially at 25...
(b) Consider an adiabatic, reversible expansion of 0 020 mol Ar (perfect gas), initially at 25 C, from 0 50 L to 1 00 L The molar heat capacity of argon is, Cvm 12 48 J K mol- Calculate the work (w) done and heat transferred (q) for this process HINT first calculate the final temperature under the adiabatic, reversible expansion process (8)
(b) Consider an adiabatic, reversible expansion of 0 020 mol Ar (perfect gas), initially at 25 C,...
By a reversible adiabatic expansion, temperature of an ideal gas (n mol) changed from T, to...
By a reversible adiabatic expansion, temperature of an ideal gas (n mol) changed from T, to Ts Express the changes of the internal energy and enthalpy by using heat capacity at conatant volume, Cy 2.
For a reversible, adiabatic expansion of 1.00 mol of a monatomic ideal gas the initial and final conditions are shown i...
For a reversible, adiabatic expansion of 1.00 mol of a monatomic ideal gas the initial and final conditions are shown in the following table and AE = W = -2.24 kJ. Initial 10.00 bar 2.478 L 298 K Final 1.00 bar 9.87 L 119 K Part A Find AH for this process. Express your answer to three significant figures and include the appropriate units. AH = Value Units Submit Request Answer
Please give detailed explanation for final part. Thanks. Reversible adiabatic expansion of ideal gas (This question...
Please give detailed explanation for final part. Thanks.
Reversible adiabatic expansion of ideal gas (This question involves working through the final section of lecture 3) Explain why the first Law for an reversible adiabatic process gives AU = -PdV, and why this equation doesn't hold for the Joule expansion. Assuming that for an ideal gas U = CVT, prove that the First Law leads to the statement that PVY is constant in a reversible adiabatic process. A container of Helium...
2 140 pt) Reversible Adiabatic Expansion of Nitrogen. Nitrogen expands reversibly in an insulated cylinder fitted...
2 140 pt) Reversible Adiabatic Expansion of Nitrogen. Nitrogen expands reversibly in an insulated cylinder fitted with a piston. The N2 is initially at 500K and 5 bar pressure and expands to a final pressure of 1 bar. Determine the final temperature T of the N2 (in K) as well as the work done in the process W (mol), assuming N2 to be in the ideal gas state. Heat capacity, Cp is equal to a constant at 3.560R.
One mole of an ideal gas undergoes a reversible adiabatic expansion from T_1, to T_2 while...
One mole of an ideal gas undergoes a reversible adiabatic expansion from T_1, to T_2 while tripling the volume of the gas. What is the relation between T_1 and T-2? T-2/3 < T_1<T_2 T_2/3 < T_1 < T-2 T_1= T_2 T_2<T_1 T_1 lessthanorequalto T_2/3 One mole of Ar gas undergoes the reversible transformation shown. Assuming Ar behaves ideally, which statement is true for step 2? Delta U= C_p DeltaT DeltaH < Delta U Delat S= c_p ln(T_c/T_B) W = etaRt...
Consider the expansion of 1.00 mole of (ideal) Ne from 2.00 atm at 75.00 C: the...
Consider the expansion of 1.00 mole of (ideal) Ne from 2.00 atm at 75.00 C: the volume is doubled in the process. Find q, w, Delta H and the final pressure and temperature for a) reversible adiabatic expansion b) reversible isothermal expansion c) reversible constant pressure expansion d) irreversible adiabat against 0.500 atm external pressure
Starting with 2.70 mol of N2 gas (assumed to be ideal) in a cylinder at 1.00...
Starting with 2.70 mol of N2 gas (assumed to be ideal) in a cylinder at 1.00 atm and 15.0 ∘C, a chemist first heats the gas at constant volume, adding 1.36 × 104 J of heat, then continues heating and allows the gas to expand at constant pressure to twice its original volume. (a) Calculate the final temperature of the gas (b) Calculate the amount of work done by the gas. (c) Calculate the amount of heat added to the...
2) Calculate w for the adiabatic expansion of 2.50 mol of an ideal gas at an...
2) Calculate w for the adiabatic expansion of 2.50 mol of an ideal gas at an initial pressure of 2.25 bar from an initial temper- ature of 450. K to a final temperature of 300. K. Write an expression for the work done in the isothermal reversible expan- sion of the gas at 300. K from an initial pressure of 2.25 bar. What value of the final pressure would give the same value of w as the first part of...
A reversible compression of 1 mol of an ideal gas in a piston/cylinder device result in...
A reversible compression of 1 mol of an ideal gas in a piston/cylinder device result in a pressure increase from 1 bar to P_2 and a temperature increase from 400 K to 950 K. The path followed by the gas during compression is given by PV^1.55 = const, and the molar heat capacity of the gas is given by C_p/R = 3.85+0.57 time sign 10^-3T [T/K] Determine the heat transferred during the process and the final pressure.
(b) Consider an adiabatic, reversible expansion of 0 020 mol Ar (perfect gas), initially at 25 C, from 0 50 L to 1 00 L The molar heat capacity of argon is, Cvm 12 48 J K mol- Calculate the work (w) done and heat transferred (q) for this process HINT first calculate the final temperature under the adiabatic, reversible expansion process (8)
(b) Consider an adiabatic, reversible expansion of 0 020 mol Ar (perfect gas), initially at 25 C,...
By a reversible adiabatic expansion, temperature of an ideal gas (n mol) changed from T, to Ts Express the changes of the internal energy and enthalpy by using heat capacity at conatant volume, Cy 2.
For a reversible, adiabatic expansion of 1.00 mol of a monatomic ideal gas the initial and final conditions are shown in the following table and AE = W = -2.24 kJ. Initial 10.00 bar 2.478 L 298 K Final 1.00 bar 9.87 L 119 K Part A Find AH for this process. Express your answer to three significant figures and include the appropriate units. AH = Value Units Submit Request Answer
Please give detailed explanation for final part. Thanks.
Reversible adiabatic expansion of ideal gas (This question involves working through the final section of lecture 3) Explain why the first Law for an reversible adiabatic process gives AU = -PdV, and why this equation doesn't hold for the Joule expansion. Assuming that for an ideal gas U = CVT, prove that the First Law leads to the statement that PVY is constant in a reversible adiabatic process. A container of Helium...
2 140 pt) Reversible Adiabatic Expansion of Nitrogen. Nitrogen expands reversibly in an insulated cylinder fitted with a piston. The N2 is initially at 500K and 5 bar pressure and expands to a final pressure of 1 bar. Determine the final temperature T of the N2 (in K) as well as the work done in the process W (mol), assuming N2 to be in the ideal gas state. Heat capacity, Cp is equal to a constant at 3.560R.
One mole of an ideal gas undergoes a reversible adiabatic expansion from T_1, to T_2 while tripling the volume of the gas. What is the relation between T_1 and T-2? T-2/3 < T_1<T_2 T_2/3 < T_1 < T-2 T_1= T_2 T_2<T_1 T_1 lessthanorequalto T_2/3 One mole of Ar gas undergoes the reversible transformation shown. Assuming Ar behaves ideally, which statement is true for step 2? Delta U= C_p DeltaT DeltaH < Delta U Delat S= c_p ln(T_c/T_B) W = etaRt...
Consider the expansion of 1.00 mole of (ideal) Ne from 2.00 atm at 75.00 C: the volume is doubled in the process. Find q, w, Delta H and the final pressure and temperature for a) reversible adiabatic expansion b) reversible isothermal expansion c) reversible constant pressure expansion d) irreversible adiabat against 0.500 atm external pressure
2) Calculate w for the adiabatic expansion of 2.50 mol of an ideal gas at an initial pressure of 2.25 bar from an initial temper- ature of 450. K to a final temperature of 300. K. Write an expression for the work done in the isothermal reversible expan- sion of the gas at 300. K from an initial pressure of 2.25 bar. What value of the final pressure would give the same value of w as the first part of...
A reversible compression of 1 mol of an ideal gas in a piston/cylinder device result in a pressure increase from 1 bar to P_2 and a temperature increase from 400 K to 950 K. The path followed by the gas during compression is given by PV^1.55 = const, and the molar heat capacity of the gas is given by C_p/R = 3.85+0.57 time sign 10^-3T [T/K] Determine the heat transferred during the process and the final pressure.
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