Question

7. A steel container, equipped with a piston, contains 21 mol of an ideal gas at 465 K. The container is compressed isothermally to 90% of its original volume. How much work is done on the gas? The ideal gas constant is R = 8.314 J/mol · K. A) 11 J B) -73,300 J C) -8500 J D) 8600 J 8. How much work is done by 3.00 mol of ideal gas when it triples its volume at a constant temperature of 127°C? The ideal gas constant is R = 8.314 J/mol · K. A) 12.7 kJ B) 11.0 kJ C) 9.97 kJ D) 15.3 kJ E) 1.20 kJ 9. An ideal gas in a balloon is kept in thermal equilibrium with its constant-temperature surroundings. How much work is done by the gas if the outside pressure is slowly reduced, allowing the balloon to expand to 6.0 times its original size? The balloon initially has a pressure of 645.0 Pa and a volume of 0.10 m³. The ideal gas constant is 8.314 J/mol · K. A) 390 J B) -330 J C) 120 J D) 6.0 J

          7. A steel container, equipped with a piston, contains 21 mol of an ideal gas at 465 K. The container is compressed isothermally to 90% of its original volume. How much work is done on the gas? The ideal gas constant is R = 8.314 J/mol · K.
A) 11 J
B) -73,300 J
C) -8500 J
D) 8600 J

8. How much work is done by 3.00 mol of ideal gas when it triples its volume at a constant temperature of 127°C? The ideal gas constant is R = 8.314 J/mol · K.
A) 12.7 kJ
B) 11.0 kJ
C) 9.97 kJ
D) 15.3 kJ
E) 1.20 kJ

9. An ideal gas in a balloon is kept in thermal equilibrium with its constant-temperature surroundings. How much work is done by the gas if the outside pressure is slowly reduced, allowing the balloon to expand to 6.0 times its original size? The balloon initially has a pressure of 645.0 Pa and a volume of 0.10 m³. The ideal gas constant is 8.314 J/mol · K.
A) 390 J
B) -330 J
C) 120 J
D) 6.0 J

Show more…

7. A steel container, equipped with a piston, contains 21 mol of an ideal gas at 465 K. The container is compressed isothermally to 90% of its original volume. How much work is done on the gas? The ideal gas constant is R = 8.314 J/mol · K.
A) 11 J
B) -73,300 J
C) -8500 J
D) 8600 J

8. How much work is done by 3.00 mol of ideal gas when it triples its volume at a constant temperature of 127°C? The ideal gas constant is R = 8.314 J/mol · K.
A) 12.7 kJ
B) 11.0 kJ
C) 9.97 kJ
D) 15.3 kJ
E) 1.20 kJ

9. An ideal gas in a balloon is kept in thermal equilibrium with its constant-temperature surroundings. How much work is done by the gas if the outside pressure is slowly reduced, allowing the balloon to expand to 6.0 times its original size? The balloon initially has a pressure of 645.0 Pa and a volume of 0.10 m³. The ideal gas constant is 8.314 J/mol · K.
A) 390 J
B) -330 J
C) 120 J
D) 6.0 J

Added by Anne W.

University Physics with Modern Physics

Hugh D. Young 14th Edition

Instant Answer

Solved by Expert Maitreya E

05/05/2022

Step 1

Given: Initial temperature, T1 = 465 K Final temperature, T2 = 465 K Initial moles of gas, n = 21 mol Compression ratio, V2/V1 = 0.9 Gas constant, R = 8.314 J/mol Using the formula for work done in an isothermal process: \[ W = -nRT \ln \left( \frac{V_f}{V_i} Show more…

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Transcript

00:01 Coming to the first problem we have given initial condition is t equal to 465 kelvin and n equal to 21 volts.

00:24 Let v1 be the volume and final condition is t is 400 and 440.

00:42 65 kelvin and v2 is 90 divided by 100 times v1.

00:51 Therefore, v2 is 0 .9 times v1.

00:59 Here, the gas is compressed isothermally.

01:16 Therefore, work done by the gas will be negative.

01:36 We have work done in isothermal process given by the formula, the w is equal to n r t1 lown of b2 divided by v1.

02:11 Substituting the values we have w is equal to 21 multiplied by 8 .314 multiplied by 465 multiplied by loan of 0 .9 times b1 divided by 3 1.

02:32 Therefore, we have w is equal to 21 multiplied by 8 .314 multiplied by 465 multiplied by lonof .9.

02:49 Simplifying we get minus 8 ,553 .8 .82 jule which can be approximated to minus 8 ,500 june.

03:08 Hence, it can be concluded that work done is equal to minus 8 ,000 ,000.

03:24 500 jules hence option c minus 8 ,500 jule is the correct answer.

03:35 Coming to the next part of the problem we have here temperature is a constant.

03:58 Therefore this is an isothermal.

04:08 Process.

04:14 Work done is given by the formula as w is equal to n rt, lohn of v2 divided by v1.

04:30 Substituting the values we have w is equal to n rt lone of v2.

04:40 Of 3 v divided by v...

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