The figure shows the variation in the internal energy $U$ with the volume $V$ of 2.0 mole of an ideal gas in a cyclic process $a b c d a$ . The temperatures of the gas at b and c are 500 K and 300 K respectively. Calculate the heat absorbed by the gas during the process.

Open in App

Solution

$Δ U = q + w$
$Δ U = 0$ (cyclic process)
$q = - w = 2 \times R (500 - 300)$
$= 2 \times 8.314 \times 200$
$= 831.4 \times 2 \times 2$
$q = - 3325.6 J$

Suggest Corrections

Similar questions

Q. Figure shows the variation in the internal energy U with the volume

V

2.0

mole of an ideal gas in a cyclic process abcda. The temperatures of the gas at

b

and

c

are

500 K

and

300 K

respectively. Calculate the heat absorbed by the gas during the process.

Figure shows the variation in the internal energy U with the volume V of 2.0 mol of an ideal gas in a cyclic process abcda. The temperatures of the gas at b and c are 500 K and 300 K respectively. Calculate the heat absorbed by the gas during the process.