Five moles of an ideal monoatomic gas with an initial temperature of `127^@C` expand and in the process absorb 1200J of heat and do 2100J of work. What is the final temperature of the gas?

Five moles of an ideal monoatomic gas with an initial temperature of 150^@C expand and in the process absorb 1500 J of heat and does 2500 J of work. The final temperature of the gas in .^@C is (ideal gas constant R = 8.314 J K^(-1)mol^(-1))

Five moles of an ideal monoatomic gas with an initial temperature of 150^@C expand and in the process absorb 1500 J of heat and does 2500 J of work. The final temperature of the gas in .^@C is (ideal gas constant R = 8.314 J K^(-1)mol^(-1))

One mole of an ideal diatomic gas absorbs 1831.4 J of heat and does 1000 J of work at 27^(@)C . What is the change in temperature observed ?

I mole of an ideal monoatomic gas is expanded till the temperature of the gas is doubled under the process V^(2)T=contant . The initial temperature of the gas is 400K . In terms of R find total work done in the process.

One mole of an ideal gas expands reversibly and adiabatically from a temperature of 27^@C . If the work done during the process is 3 kJ, then final temperature of the gas is ( C_V = 20 J/K )

For monoatomic gas, its initial temperature 127° C if adiabatically its volume changed to 8/27 of its initial value then what will be final temperature

The work done by an ideal gas at constant temperature is 10 J. the amount of heat gained in this process is

One mole of an ideal monoatomic gas at temperature T_0 expands slowly according to the law p/V = constant. If the final temperature is 2T_0 , heat supplied to the gas is