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.

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 127^@C expand and in the process absorb 1200J of heat and do 2100J of work. What is the final temperature of the gas?

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 )

Two moles of an ideal monoatomic gas occupy a volume 2V at temperature 300K, it expands to a volume 4V adiabatically, then the final temperature of gas is

Two moles of an ideal monoatomic gas occupy a volume 2V at temperature 300K, it expands to a volume 4V adiabatically, then the final temperature of gas is

The initial temperature of a two mole monoatomic gas is T. If temperature increases to 3T then work done in the adiabatic process is

If 4 moles of an ideal monoatomic gas at temperature 400 K is mixed with 2 mole of another ideal monoatomic gas at temperature 700 K, the temperature of the mixture is

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))