Question

When heat Q is supplied to a diatomic gas of rigid molecules at constant volume its temperature increases by ∆T. The heat required to produce the same change in temperature, at constant pressure is :
(A) (3/2)Q (B) (5/3)Q (C) (7/5)Q (D) (2/3)Q

Answer 1

Explanation:

.(D) ., (2/ 3 )Q...... ..

Answer 2

The heat required to produce the same change in temperature, at constant pressure = $\frac{7}{5}$

Given:

Heat Q is supplied to a diatomic gas of rigid molecules at constant volume its temperature increases by ∆T.

To find:

The heat required to produce the same change in temperature, at constant pressure.

Formula used:

For diatomic gas.

$C_{p}$ = $\frac{7R}{2}$   $C_{v}$ = $\frac{5R}{2}$    

Heat supplied at constant volume = m$C_{v}$ dt

Heat supplied at constant volume = m$C_{p}$ dt

Explanation:

$\frac{Heat \ supplied\ at\ constant\ pressure }{Heat\ supplied\ at\ constant\ volume}$ = $\frac{mC_{p} dt }{ mC_{v}dt }$

$\frac{Heat \ supplied\ at\ constant\ pressure }{Heat\ supplied\ at\ constant\ volume}$ = $\frac{C_p}{C_v}$

$\frac{Heat \ supplied\ at\ constant\ pressure }{Heat\ supplied\ at\ constant\ volume}$ = $\frac{\frac{7R}{2}}{\frac{5R}{2}}$

$\frac{Heat \ supplied\ at\ constant\ pressure }{Heat\ supplied\ at\ constant\ volume}$ = $\frac{7}{5}$

The heat required to produce the same change in temperature, at constant pressure =  $\frac{7}{5}$

To learn more....

1)1) A diatomic ideal gas is heated at constant volume until its pressure is doubled. It is again heated at constant pressure until its volume is doubled. The molar heat capacity for the whole process is kR. Find the value of k.

brainly.in/question/109810

2)70 calories are required to raise the temperature of 2 moles of an ideal gas at constant pressure from 30°C to 35°C.The amount of heat required (in calories) to raise the temperature of the same gas through the same range (30°C to 35°C) at constant volume is?

brainly.in/question/109810