In a process `V prop T^(2)`, temperature of 2 moles of a gas is increased by 200K. Work done by the gas in this process will be

Assertion: In the process pT=constant, if temperature of gas is increased work done by the gas is positive. Reason: For the given process, VpropT .

Assertion: In the process pT=constant, if temperature of gas is increased work done by the gas is positive. Reason: For the given process, VpropT .

One mole of an ideal monoatomic gas under goes a process V=aT^(2) . The temperature of the gas increases by 100 K . Which of the following is incorrect ?

One mole of an ideal monoatomic gas under goes a process V=aT^(2) . The temperature of the gas increases by 100 K . Which of the following is incorrect ?

During adiabatic expansion of 2 moles of a gas, the internal energy of the gas is found to decrease by 2J. The work done by the gas during the process is

A sample of ideal gas is taken through the cyclic process shown in the figure. The temerauture of the gas in state A is T_(A) =200 K. In states B and C the temperature of the gas is the same. Net work done by the gas in the process is

A sample of ideal gas is taken through the cyclic process shown in the figure. The temerauture of the gas in state A is T_(A) =200 K. In states B and C the temperature of the gas is the same. Net work done by the gas in the process 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

Method 1 of Q Temperature of two moles of a monoatomic gas is increased by 300 K in the process p prop V . (a) Find molar heat capacity of the gas in the given process. (b) Find heat given to the gas in that.

In a thermodynamic process two moles of a monatomic ideal gas obeys PV^(–2)=constant . If temperature of the gas increases from 300 K to 400 K, then find work done by the gas (Where R = universal gas constant)