Question

A sample of xenon gas at a pressure of 817 mm Hg and a temperature of 66 °C, occupies a volume of 13.9 liters. If the gas is heated at constant pressure to a temperature of 89 °C, the volume of the gas sample will be 14.84 L.

Answer 1

Answer:

The value of heat transfer in xenon gas during heating at constant pressure  Q = 0.254  KJ

Explanation:

Initial pressure $P_{1}$ = 109 k pa = Final pressure

Initial temperature $T_{1}$ = 66°c = 339 K

Initial volume $V_{1}$ = 13.9 liter = 0.0139 $m^{3}$

Final temperature $T_{2}$ = 362 K

Final volume $V_{2}$ = 14.84 liter

Specific heat for xenon at constant pressure $C_{p}$ = 0.158 $\frac{KJ}{kg K}$

Gas constant  for xenon (R)= 0.063 $\frac{KJ}{kg K}$

From ideal gas equation

$P_{1}$ $V_{1}$ = m R $T_{1}$------ (1)

⇒ 109 × 0.0139 = m × 0.06333 × 339

⇒ m = 0.07 kg

This is the mass of xenon gas.

heat transfer is given by

$Q = m C_{p} ( T_{2} - T_{1} )$

Put all the value sin above equation we get

Q = 0.07 × 0.158 × (362 - 339)

Q = 0.254  KJ

This is the value of heat transfer in xenon gas during heating at constant pressure.