Question

The maximum work done is obtained when pressure on 10 g of hydrogen is reduced from 20 to 1 ATM at a constant temperature of 300 k. The gas behaves ideally. The value of q is

Answer 1

Answer:The maximum work done is  -8970 calories.

Explanation:

This is the case of isothermal reversible expansion of gas.

Formula used :

w=-2.303nRTlog(p1/p2)

where,

w = work done by the gas

n = number of moles of gas

R = gas constant =  1.9872 cal/K·mol

T = temperature of gas = 300 K

m = mass of hydrogen gas = 10 g

M = molar mass of hydrogen gas,  = 2 g/mole

P1 = initial pressure of gas = 20 atm

P2 = final pressure of gas = 1 atm

Now put all the given values in the above formula, we get the work done.

Therefore, the maximum work done is -8970calories