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
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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
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