139359 One mole of an ideal gas requires $207 \mathrm{~J}$ heat to raise the temperature by $10 \mathrm{~K}$ when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by the same $10 \mathrm{~K}$, the heat required is (Given the gas constant $R=8.3 \mathrm{~J} / \mathrm{mol}-\mathrm{K})$

139360 For a certain gas the ratio of specific heats is given to be $\gamma=1.5$, for this gas

139361 For hydrogen gas $C_{p}-C_{v}=a$ and for oxygen gas $C_{p}-C_{v}=b$, so the relation between a and $b$ is given by

139362 The molar specific heats of an ideal gas at constant pressure and volume are denoted by $C_{p}$ and $C_{V}$ respectively. If $\gamma=\frac{C_{p}}{C_{v}}$ and $R$ is the universal gas constant, then $C_{V}$ is equal to

139359 One mole of an ideal gas requires $207 \mathrm{~J}$ heat to raise the temperature by $10 \mathrm{~K}$ when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by the same $10 \mathrm{~K}$, the heat required is (Given the gas constant $R=8.3 \mathrm{~J} / \mathrm{mol}-\mathrm{K})$

139360 For a certain gas the ratio of specific heats is given to be $\gamma=1.5$, for this gas

139361 For hydrogen gas $C_{p}-C_{v}=a$ and for oxygen gas $C_{p}-C_{v}=b$, so the relation between a and $b$ is given by

139362 The molar specific heats of an ideal gas at constant pressure and volume are denoted by $C_{p}$ and $C_{V}$ respectively. If $\gamma=\frac{C_{p}}{C_{v}}$ and $R$ is the universal gas constant, then $C_{V}$ is equal to

139359 One mole of an ideal gas requires $207 \mathrm{~J}$ heat to raise the temperature by $10 \mathrm{~K}$ when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by the same $10 \mathrm{~K}$, the heat required is (Given the gas constant $R=8.3 \mathrm{~J} / \mathrm{mol}-\mathrm{K})$

139360 For a certain gas the ratio of specific heats is given to be $\gamma=1.5$, for this gas

139361 For hydrogen gas $C_{p}-C_{v}=a$ and for oxygen gas $C_{p}-C_{v}=b$, so the relation between a and $b$ is given by

139362 The molar specific heats of an ideal gas at constant pressure and volume are denoted by $C_{p}$ and $C_{V}$ respectively. If $\gamma=\frac{C_{p}}{C_{v}}$ and $R$ is the universal gas constant, then $C_{V}$ is equal to

139359 One mole of an ideal gas requires $207 \mathrm{~J}$ heat to raise the temperature by $10 \mathrm{~K}$ when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by the same $10 \mathrm{~K}$, the heat required is (Given the gas constant $R=8.3 \mathrm{~J} / \mathrm{mol}-\mathrm{K})$

139360 For a certain gas the ratio of specific heats is given to be $\gamma=1.5$, for this gas

139361 For hydrogen gas $C_{p}-C_{v}=a$ and for oxygen gas $C_{p}-C_{v}=b$, so the relation between a and $b$ is given by

139362 The molar specific heats of an ideal gas at constant pressure and volume are denoted by $C_{p}$ and $C_{V}$ respectively. If $\gamma=\frac{C_{p}}{C_{v}}$ and $R$ is the universal gas constant, then $C_{V}$ is equal to