What will be the value of maximum work one by the gas when pressure of 20 gm `H_(2)` is reduced from 20 to 2 atm at constant tempreature of 300 k, assuming gas to behave ideally?

Calculate the maximum work done by an ideal gas when pressure on 10 g of H_2 is reduced from 20 to 2 atm at a constant temperature 300 K.

The maximum work done when pressure on 10 g of hydrogen is reduced from 20 to 1 atm at a constant temeprature of 273 will be

The maximum work done when pressure of n moles of H_(2) was reduced from 20 atm to 1 atm at constant temperature of 273 K is found to be 8180 calories. What is the value of n?

The maximum work done when pressure of n moles of H_(2) was reduced from 20 atm to 1 atm at constant temperature of 273 K is found to be 8180 calories. What is the value of n?

Calculate the maximum work done when pressure on 10 g of hydrogen is reduces from 20 atm to 1 atm at a constant temperature of 273 K . The gas behaves ideally. Will there be any change in internal energy? Also, calculate 'q' .

Calculate the maximum work down when pressure on 10g of hydrogen is reduced from 20 to 1atm at a constant temperature of 273K . The gas behaves ideally. Will there be any change in internal energy. Also calculate q. (R = 2 cal K^(-1) mol^(-1))

Calculate the maximum work down when pressure on 10g of hydrogen is reduced from 20 to 1atm at a constant temperature of 273K . The gas behaves ideally. Will there be any change in internal energy. Also calculate q. (R = 2 cal K^(-1) mol^(-1))

Calculate work done when 1 mole of an ideal gas is expanded reversibly from 20 L to 40 L at a constant temperature of 300 K.

What work will be done, when 3 moles of an ideal gas are compreseed to half the initial volume at a constant temperature of 300K?