139130 The r.m.s speed of molecules of an ideal gas at $27^{\circ} \mathrm{C}$ is $200 \mathrm{~ms}^{-1}$, when the temperature is increased to $327^{\circ} \mathrm{C}$, the r.m.s. speed of the molecules is changed to

139132 A vessel containing nitrogen gas is supplied a heat of $498 \mathrm{~J}$, so as to raise the temperature of the gas by $40^{\circ} \mathrm{C}$ at constant pressure. The mass of nitrogen gas in the vessel is
(Molecular mass of nitrogen $=\mathbf{2 8} \mathrm{g}$; Universal gas constant $=8.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$ )

139136 Two boxes are at the same temperature. The first box contains gas with molecular mass $m_{1}$ and rms speed $v_{1}$. The second box contains gas with molecular mass $m_{2}$ and average speed $v_{2}$.
$\text { If } \mathrm{v}_{1}=1.5 \mathrm{v}_{2} \text {, then } \frac{\mathrm{m}_{1}}{\mathrm{~m}_{2}} \text { is - }$

139138 The rms speed of oxygen at room temperature is about $500 \mathrm{~ms}^{-1}$. The rms speed of hydrogen at the same temperature is about.

139139 A gas has $n$ degrees of freedom. The ratio of specific heat of gas at constant volume to the specific heat of gas at constant pressure will be:

139130 The r.m.s speed of molecules of an ideal gas at $27^{\circ} \mathrm{C}$ is $200 \mathrm{~ms}^{-1}$, when the temperature is increased to $327^{\circ} \mathrm{C}$, the r.m.s. speed of the molecules is changed to

139132 A vessel containing nitrogen gas is supplied a heat of $498 \mathrm{~J}$, so as to raise the temperature of the gas by $40^{\circ} \mathrm{C}$ at constant pressure. The mass of nitrogen gas in the vessel is
(Molecular mass of nitrogen $=\mathbf{2 8} \mathrm{g}$; Universal gas constant $=8.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$ )

139136 Two boxes are at the same temperature. The first box contains gas with molecular mass $m_{1}$ and rms speed $v_{1}$. The second box contains gas with molecular mass $m_{2}$ and average speed $v_{2}$.
$\text { If } \mathrm{v}_{1}=1.5 \mathrm{v}_{2} \text {, then } \frac{\mathrm{m}_{1}}{\mathrm{~m}_{2}} \text { is - }$

139138 The rms speed of oxygen at room temperature is about $500 \mathrm{~ms}^{-1}$. The rms speed of hydrogen at the same temperature is about.

139139 A gas has $n$ degrees of freedom. The ratio of specific heat of gas at constant volume to the specific heat of gas at constant pressure will be:

139130 The r.m.s speed of molecules of an ideal gas at $27^{\circ} \mathrm{C}$ is $200 \mathrm{~ms}^{-1}$, when the temperature is increased to $327^{\circ} \mathrm{C}$, the r.m.s. speed of the molecules is changed to

139132 A vessel containing nitrogen gas is supplied a heat of $498 \mathrm{~J}$, so as to raise the temperature of the gas by $40^{\circ} \mathrm{C}$ at constant pressure. The mass of nitrogen gas in the vessel is
(Molecular mass of nitrogen $=\mathbf{2 8} \mathrm{g}$; Universal gas constant $=8.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$ )

139136 Two boxes are at the same temperature. The first box contains gas with molecular mass $m_{1}$ and rms speed $v_{1}$. The second box contains gas with molecular mass $m_{2}$ and average speed $v_{2}$.
$\text { If } \mathrm{v}_{1}=1.5 \mathrm{v}_{2} \text {, then } \frac{\mathrm{m}_{1}}{\mathrm{~m}_{2}} \text { is - }$

139138 The rms speed of oxygen at room temperature is about $500 \mathrm{~ms}^{-1}$. The rms speed of hydrogen at the same temperature is about.

139139 A gas has $n$ degrees of freedom. The ratio of specific heat of gas at constant volume to the specific heat of gas at constant pressure will be:

139130 The r.m.s speed of molecules of an ideal gas at $27^{\circ} \mathrm{C}$ is $200 \mathrm{~ms}^{-1}$, when the temperature is increased to $327^{\circ} \mathrm{C}$, the r.m.s. speed of the molecules is changed to

139132 A vessel containing nitrogen gas is supplied a heat of $498 \mathrm{~J}$, so as to raise the temperature of the gas by $40^{\circ} \mathrm{C}$ at constant pressure. The mass of nitrogen gas in the vessel is
(Molecular mass of nitrogen $=\mathbf{2 8} \mathrm{g}$; Universal gas constant $=8.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$ )

139136 Two boxes are at the same temperature. The first box contains gas with molecular mass $m_{1}$ and rms speed $v_{1}$. The second box contains gas with molecular mass $m_{2}$ and average speed $v_{2}$.
$\text { If } \mathrm{v}_{1}=1.5 \mathrm{v}_{2} \text {, then } \frac{\mathrm{m}_{1}}{\mathrm{~m}_{2}} \text { is - }$

139138 The rms speed of oxygen at room temperature is about $500 \mathrm{~ms}^{-1}$. The rms speed of hydrogen at the same temperature is about.

139139 A gas has $n$ degrees of freedom. The ratio of specific heat of gas at constant volume to the specific heat of gas at constant pressure will be:

139130 The r.m.s speed of molecules of an ideal gas at $27^{\circ} \mathrm{C}$ is $200 \mathrm{~ms}^{-1}$, when the temperature is increased to $327^{\circ} \mathrm{C}$, the r.m.s. speed of the molecules is changed to

139132 A vessel containing nitrogen gas is supplied a heat of $498 \mathrm{~J}$, so as to raise the temperature of the gas by $40^{\circ} \mathrm{C}$ at constant pressure. The mass of nitrogen gas in the vessel is
(Molecular mass of nitrogen $=\mathbf{2 8} \mathrm{g}$; Universal gas constant $=8.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$ )

139136 Two boxes are at the same temperature. The first box contains gas with molecular mass $m_{1}$ and rms speed $v_{1}$. The second box contains gas with molecular mass $m_{2}$ and average speed $v_{2}$.
$\text { If } \mathrm{v}_{1}=1.5 \mathrm{v}_{2} \text {, then } \frac{\mathrm{m}_{1}}{\mathrm{~m}_{2}} \text { is - }$

139138 The rms speed of oxygen at room temperature is about $500 \mathrm{~ms}^{-1}$. The rms speed of hydrogen at the same temperature is about.

139139 A gas has $n$ degrees of freedom. The ratio of specific heat of gas at constant volume to the specific heat of gas at constant pressure will be: