148256 A gas is suddenly expanded such that its final volume becomes 3 times its initial volume. If the specific heat at constant volume of the gas is $2 \mathrm{R}$, then the ratio of initial to final pressures is nearly equal to

148257 An ideal gas expands along the path $\mathrm{AB}$ as shown in the p-V diagram. The work done is

148259 One mole of nitrogen gas being initially at a temperature of $T_{0}=300 \mathrm{~K}$ is adiabatically compressed to increase its pressure 10 times. The final gas temperature after compression is (Assume, nitrogen gas molecules as rigid diatomic and $100^{1 / 7}=1.9$ )

148260 A diesel engine has a compression ratio of 20 :1. If the initial pressure is $1 \times 10^{5} \mathrm{~Pa}$ and the initial volume of the cylinder is $1 \times 10^{-3} \mathrm{~m}^{3}$, then how much work does the gas do during the compression?
(Assume the process as adiabatic)
$\left(C_{v}=20.8 \mathrm{~J} / \mathrm{mol} \mathrm{K}, \gamma_{\text {air }}=1.4,(20)^{1.4}=66.3\right)$

148256 A gas is suddenly expanded such that its final volume becomes 3 times its initial volume. If the specific heat at constant volume of the gas is $2 \mathrm{R}$, then the ratio of initial to final pressures is nearly equal to

148257 An ideal gas expands along the path $\mathrm{AB}$ as shown in the p-V diagram. The work done is

148259 One mole of nitrogen gas being initially at a temperature of $T_{0}=300 \mathrm{~K}$ is adiabatically compressed to increase its pressure 10 times. The final gas temperature after compression is (Assume, nitrogen gas molecules as rigid diatomic and $100^{1 / 7}=1.9$ )

148260 A diesel engine has a compression ratio of 20 :1. If the initial pressure is $1 \times 10^{5} \mathrm{~Pa}$ and the initial volume of the cylinder is $1 \times 10^{-3} \mathrm{~m}^{3}$, then how much work does the gas do during the compression?
(Assume the process as adiabatic)
$\left(C_{v}=20.8 \mathrm{~J} / \mathrm{mol} \mathrm{K}, \gamma_{\text {air }}=1.4,(20)^{1.4}=66.3\right)$

148256 A gas is suddenly expanded such that its final volume becomes 3 times its initial volume. If the specific heat at constant volume of the gas is $2 \mathrm{R}$, then the ratio of initial to final pressures is nearly equal to

148257 An ideal gas expands along the path $\mathrm{AB}$ as shown in the p-V diagram. The work done is

148259 One mole of nitrogen gas being initially at a temperature of $T_{0}=300 \mathrm{~K}$ is adiabatically compressed to increase its pressure 10 times. The final gas temperature after compression is (Assume, nitrogen gas molecules as rigid diatomic and $100^{1 / 7}=1.9$ )

148260 A diesel engine has a compression ratio of 20 :1. If the initial pressure is $1 \times 10^{5} \mathrm{~Pa}$ and the initial volume of the cylinder is $1 \times 10^{-3} \mathrm{~m}^{3}$, then how much work does the gas do during the compression?
(Assume the process as adiabatic)
$\left(C_{v}=20.8 \mathrm{~J} / \mathrm{mol} \mathrm{K}, \gamma_{\text {air }}=1.4,(20)^{1.4}=66.3\right)$

148256 A gas is suddenly expanded such that its final volume becomes 3 times its initial volume. If the specific heat at constant volume of the gas is $2 \mathrm{R}$, then the ratio of initial to final pressures is nearly equal to

148257 An ideal gas expands along the path $\mathrm{AB}$ as shown in the p-V diagram. The work done is

148259 One mole of nitrogen gas being initially at a temperature of $T_{0}=300 \mathrm{~K}$ is adiabatically compressed to increase its pressure 10 times. The final gas temperature after compression is (Assume, nitrogen gas molecules as rigid diatomic and $100^{1 / 7}=1.9$ )

148260 A diesel engine has a compression ratio of 20 :1. If the initial pressure is $1 \times 10^{5} \mathrm{~Pa}$ and the initial volume of the cylinder is $1 \times 10^{-3} \mathrm{~m}^{3}$, then how much work does the gas do during the compression?
(Assume the process as adiabatic)
$\left(C_{v}=20.8 \mathrm{~J} / \mathrm{mol} \mathrm{K}, \gamma_{\text {air }}=1.4,(20)^{1.4}=66.3\right)$