For an isobaric process,the ratio of `Delta Q` (amount of heat supplied) to the `Delta ` (work done by the gas) is `(gamma=(C_(P))/(C_(v)))`

In an isobaric process, the ratio of heat supplied to the system (dQ) and work done by the system (dW) for diatomic gas is

For adiabatic processes (gamma = (C_(p))/(C_(v)))

In an isobaric process of an ideal gas. The ratio of heat supplied annd work done by the system [i.e.,((Q)/(W))] is

A sample of ideal gas (gamma=1.4) is heated at constant pressure. If an amount of 100 J heat is supplied to the gas, the work done by the gas is

P_(i), V_(i) are initial pressure and volumes and V_(f) is final volume of a gas in a thermodynamic process respectively. If PV^(n) = constant, then the amount of work done by gas is : (gamma = C_(p)//C_(v)) . Assume same, initial states & same final volume in all processes.

A sample of an ideal diatomic gas is heated at constant pressure. If an amount of 100 J of heat is supplied to the gas, find the work done by the gas.

In a process, the molar heat capacity of a diatomic gas is (10)/(3) R . When heat Q is supplied to the gas, find the work done by the gas

Let Q and W denote the amount of heat given to an ideal gas the work done by it in an isothermal process.