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A container holds 1.0 g of argon at a pressure of 8.0
Chapter 17, Problem 21E(choose chapter or problem)
Problem 21E
A container holds 1.0 g of argon at a pressure of 8.0 atm.
a. How much heat is required to increase the temperature by 100°C at constant volume?
b. How much will the temperature increase if this amount of heat energy is transferred to the gas at constant pressure?
Questions & Answers
QUESTION:
Problem 21E
A container holds 1.0 g of argon at a pressure of 8.0 atm.
a. How much heat is required to increase the temperature by 100°C at constant volume?
b. How much will the temperature increase if this amount of heat energy is transferred to the gas at constant pressure?
ANSWER:
Step 1 of 2
a.) We need to find out the amount of heat required to increase the temperature by \(100^{\circ} \mathrm{C}\) at constant volume.
The number of moles of argon gas in the container is given by,
\(n=\frac{M}{M_{m o l}}\)
The atomic mass of argon, \(M_{m o l}=40 \mathrm{~g} / \mathrm{mol}\)
So,
\(n =\frac{1 g}{40 g / m o l}\)
\(n =0.025 \mathrm{~mol}\)
The amount of heat required to increase the temperature by \(100^{\circ} \mathrm{C}\) at constant volume is given by.
\(Q=n c_{v} \Delta T\)
\(Q=(0.025 \mathrm{~mol})(12.5 \mathrm{~J} / \mathrm{kg} \mathrm{K})\left(100^{0} \mathrm{C}\right)\)
\(Q=31.25 \mathrm{~J}\)