148301 The figure below shows the plot of $\frac{P V}{n T}$ versus $P$ for oxygen gas at two different temperatures

Read the following statements concerning the above curves :
(i) The dotted line corresponds to the ideal gas behaviour.
(ii) $\mathrm{T}_{1}>\mathrm{T}_{2}$
(iii) The value of $\mathrm{PV} / \mathrm{nT}$ at the point where the curves meet on the $y$-axis is the same for all gases.
Which of the above statements is true ?

148302 The following figure represents the temperature versus time plot for a given amount of a substance when heat energy is supplied to it at a fixed rate and at constant pressure.

Which parts of the above plot represent a phase change ?

148303 The work done, $W$ during an isothermal process in which 1 mole of the gas expands from an initial volume $V_{1}$ to a final volume $V_{2}$ is given by: $(R=$ gas constant, $T=$ temperature $)$

148305 The pressure and density of a diatomic gas $\left(\gamma=\frac{7}{5}\right)$ change adiabatically from $(P, d)$ to $\left(P^{\prime} d^{\prime}\right)$. If $\frac{d^{\prime}}{d}=32$, then $\frac{P^{\prime}}{P}$ should be :

148306 A gas at NTP is suddenly compressed to onefourth of its original volume. If $\gamma$ is supposed to be $3 / 2$, then the final pressure is :

148301 The figure below shows the plot of $\frac{P V}{n T}$ versus $P$ for oxygen gas at two different temperatures

Read the following statements concerning the above curves :
(i) The dotted line corresponds to the ideal gas behaviour.
(ii) $\mathrm{T}_{1}>\mathrm{T}_{2}$
(iii) The value of $\mathrm{PV} / \mathrm{nT}$ at the point where the curves meet on the $y$-axis is the same for all gases.
Which of the above statements is true ?

148302 The following figure represents the temperature versus time plot for a given amount of a substance when heat energy is supplied to it at a fixed rate and at constant pressure.

Which parts of the above plot represent a phase change ?

148303 The work done, $W$ during an isothermal process in which 1 mole of the gas expands from an initial volume $V_{1}$ to a final volume $V_{2}$ is given by: $(R=$ gas constant, $T=$ temperature $)$

148305 The pressure and density of a diatomic gas $\left(\gamma=\frac{7}{5}\right)$ change adiabatically from $(P, d)$ to $\left(P^{\prime} d^{\prime}\right)$. If $\frac{d^{\prime}}{d}=32$, then $\frac{P^{\prime}}{P}$ should be :

148306 A gas at NTP is suddenly compressed to onefourth of its original volume. If $\gamma$ is supposed to be $3 / 2$, then the final pressure is :

148301 The figure below shows the plot of $\frac{P V}{n T}$ versus $P$ for oxygen gas at two different temperatures

Read the following statements concerning the above curves :
(i) The dotted line corresponds to the ideal gas behaviour.
(ii) $\mathrm{T}_{1}>\mathrm{T}_{2}$
(iii) The value of $\mathrm{PV} / \mathrm{nT}$ at the point where the curves meet on the $y$-axis is the same for all gases.
Which of the above statements is true ?

148302 The following figure represents the temperature versus time plot for a given amount of a substance when heat energy is supplied to it at a fixed rate and at constant pressure.

Which parts of the above plot represent a phase change ?

148303 The work done, $W$ during an isothermal process in which 1 mole of the gas expands from an initial volume $V_{1}$ to a final volume $V_{2}$ is given by: $(R=$ gas constant, $T=$ temperature $)$

148305 The pressure and density of a diatomic gas $\left(\gamma=\frac{7}{5}\right)$ change adiabatically from $(P, d)$ to $\left(P^{\prime} d^{\prime}\right)$. If $\frac{d^{\prime}}{d}=32$, then $\frac{P^{\prime}}{P}$ should be :

148306 A gas at NTP is suddenly compressed to onefourth of its original volume. If $\gamma$ is supposed to be $3 / 2$, then the final pressure is :

148301 The figure below shows the plot of $\frac{P V}{n T}$ versus $P$ for oxygen gas at two different temperatures

Read the following statements concerning the above curves :
(i) The dotted line corresponds to the ideal gas behaviour.
(ii) $\mathrm{T}_{1}>\mathrm{T}_{2}$
(iii) The value of $\mathrm{PV} / \mathrm{nT}$ at the point where the curves meet on the $y$-axis is the same for all gases.
Which of the above statements is true ?

148302 The following figure represents the temperature versus time plot for a given amount of a substance when heat energy is supplied to it at a fixed rate and at constant pressure.

Which parts of the above plot represent a phase change ?

148303 The work done, $W$ during an isothermal process in which 1 mole of the gas expands from an initial volume $V_{1}$ to a final volume $V_{2}$ is given by: $(R=$ gas constant, $T=$ temperature $)$

148305 The pressure and density of a diatomic gas $\left(\gamma=\frac{7}{5}\right)$ change adiabatically from $(P, d)$ to $\left(P^{\prime} d^{\prime}\right)$. If $\frac{d^{\prime}}{d}=32$, then $\frac{P^{\prime}}{P}$ should be :

148306 A gas at NTP is suddenly compressed to onefourth of its original volume. If $\gamma$ is supposed to be $3 / 2$, then the final pressure is :

148301 The figure below shows the plot of $\frac{P V}{n T}$ versus $P$ for oxygen gas at two different temperatures

Read the following statements concerning the above curves :
(i) The dotted line corresponds to the ideal gas behaviour.
(ii) $\mathrm{T}_{1}>\mathrm{T}_{2}$
(iii) The value of $\mathrm{PV} / \mathrm{nT}$ at the point where the curves meet on the $y$-axis is the same for all gases.
Which of the above statements is true ?

148302 The following figure represents the temperature versus time plot for a given amount of a substance when heat energy is supplied to it at a fixed rate and at constant pressure.

Which parts of the above plot represent a phase change ?

148303 The work done, $W$ during an isothermal process in which 1 mole of the gas expands from an initial volume $V_{1}$ to a final volume $V_{2}$ is given by: $(R=$ gas constant, $T=$ temperature $)$

148305 The pressure and density of a diatomic gas $\left(\gamma=\frac{7}{5}\right)$ change adiabatically from $(P, d)$ to $\left(P^{\prime} d^{\prime}\right)$. If $\frac{d^{\prime}}{d}=32$, then $\frac{P^{\prime}}{P}$ should be :

148306 A gas at NTP is suddenly compressed to onefourth of its original volume. If $\gamma$ is supposed to be $3 / 2$, then the final pressure is :