An ideal monoatomic gas at temperature `27^@C` and pressure `10^6N//m^2` occupies 10L volume. 10,000 cal of heat is added to the system without changing the volume. Calculate the change in temperature of the gas. Given : `R=8.31 J//mol-K` and `J=4.18J//cal.`

If 50 cal of heat is supplied to the system containing 2 mol of an ideal monatomic gas, the rise in temperature is (R = 2 cal//mol-K)

If 50 cal of heat is supplied to the system containing 2 mol of an ideal monatomic gas, the rise in temperature is (R = 2 cal//mol-K)

If 50 cal of heat is supplied at constant pressure to the system containing 2 mol of an ideal monatomic gas, the rise in temperature is (R = 2 cal//mol-K)

At 27^@C two moles of an ideal monatomic gas occupy a volume V. The gas expands adiabatically to a volume 2V . Calculate (a) final temperature of the gas (b) change in its internal energy and [ R=8.31J//mol-K ]

A gas is compressed at a constant pressure of 50N/m^(2) from a volume 10m^(3) to a volume of 6m^(3) . 100J of heat is added to the gas then its internal energy increases by - - in J ?

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))

The molar specific heat of an ideal gas at constant pressure is C_(p) = 5/2 R . Some amount of this gas in a closed container has a volume 0.0083 m^(3) , a temperature 300 K and a pressure 1.6 xx 10^(6) N cdot m^(-2) . If 2.49 xx 10^(4) J 1 of heat is supplied at a constant volume of the gas, find out the final temperature and pressure. Given, R = 8.3 J cdot mol^(-1) cdot K^(-1) .

A gas expands against a constant pressure of 1 atm from a volume of 5L to 10L. During the process, system absorbs 400 J of heat from the surroundings. Calculate the change in the internal energy of the system.

A gaseous system absorbs 450 cal heat. The work done by the system is 836.2 J. Find the change in internal energy of the gas in calorie. (J=4.186 J "cal"^(-1) )