Question 740: Thermodynamics & KTG

Question

The internal energy of an ideal diatomic gas corresponding to volume ' $V$ ' and pressure ' P ' is 2.5 PV. The gas expands from 1 litre to 2 litre at a constant pressure of $10^5 \mathrm{~N} / \mathrm{m}^2$. The heat supplied to a gas is

Accepted Answer

To determine the heat supplied to the ideal diatomic gas, we use the relation:
$ Q = \Delta U + W $
Where $ Q $ is the heat supplied, $ \Delta U $ is the change in internal energy, and $ W $ is the work done on the system. Given that the internal energy of the gas is $ 2.5 PV $, the work done by the gas during expansion at constant pressure can be expressed as $ PV $.
Thus:
$ Q = 2.5 PV + PV = 3.5 PV $
Substitute the given pressure ($ P = 10^5 \, \mathrm{N/m}^2 $) into the equation:
$ Q = 3.5 	imes 10^5 = 350 \, \mathrm{J} $
Hence, the heat supplied to the gas is 350 J.

Answer

350 J

Answer

300 J

Answer

250 J

Answer

200 J

Thermodynamics & KTG

The internal energy of an ideal diatomic gas corresponding to volume ' V ' and pressure ' P ' is 2.5 PV. The gas expands from 1 litre to 2 litre at a constant pressure of 10^5 \mathrm{~N} / \mathrm{m}^2. The heat supplied to a gas is

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