Question

n-moles of an ideal gas with constant volume heat capacity Cᵥ undergo an isobaric expansion by certain volume. The ratio of the work done in the process, to the heat supplied is
(A) nR/(Cᵥ - nR)
(B) nR/(Cᵥ + nR)
(C) 4nR/(Cᵥ + nR)
(D) 4nR/(Cᵥ - nR)

Answer 1

The ratio of the work done in the process, to the heat supplied =  $\frac{nR}{C_v+nR}$  

Given:

n-moles of an ideal gas with constant volume heat capacity Cᵥ undergo an isobaric expansion by certain volume.

Find:

The ratio of the work done in the process, to the heat supplied.

Formula used:

In isobaric process W = nRdT

                                Q= n$C_p$dT

 Where W= work done.

             Q= Heat supplied.

            dT = change in temperature.

            R = Universal gas constant.

Explanation:

$\frac{Work\ done}{Heat \ supplied}$ =  $\frac{nRdT}{nC_p dT}$

$\frac{Work\ done}{Heat \ supplied}$ = $\frac{R}{C_p}$ = $\frac{R}{C_v+R}$            Where,  $C_p$ = Cᵥ +R

$\frac{Work\ done}{Heat \ supplied}$ = $\frac{nR}{nC_v+nR}$        Multiply numerator and denominator by "n"      

$\frac{Work\ done}{Heat \ supplied}$ = $\frac{nR}{C_v+nR}$  

To learn more....

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.

https://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?

https://brainly.in/question/109810