Explain the effect of increasing the temperature of a liquid, on intermolecular forces operating between its particles. What will happen to the viscosity of a liquid if its temperature is increased?
As the temperature of a liquid increases, kinetic energy of the molecules increases which can overcome intermolecular forces. So, the liquid can flow more easily, this results in decrease in viscosity of the liquid.
The variation of pressure with volume of the gas at different temperatures can be graphically represented as shown in figure. On the basis of this graph answer the following questions.
(i) How will the volume of a gas change if its pressure is increased at constant temperature?
(ii) At a constant pressure, how will the volume of a gas change if the temperature is increased from 200 K to 400 K ?
(i) In accordance to Boyle's law, pressure of a gas is inversly proportional to its volume if temperature is kept constant. Thus, the volume of a gas will decrease if the pressure on the gas is increased keeping the temperature constant. e.g., at 200 K when pressure increases from $p_1$ to $p_2$, volume of the gas decreases, $V_2
(ii) In accordance to Charles law, volume of a gas is directly proportional to its temperature if pressure is kept constant.
Thus, on increasing temperature, the volume of a gas will increase if pressure is kept constant.
At constant $p$ when we increase the temperature from 200 K to 400 K , the volume of the gas increases, $V_4>V_3$.
Pressure versus volume graph for a real gas and an ideal gas are shown in figure. Answer the following questions on the basis of this graph.
(i) Interpret the behaviour of real gas with respect to ideal gas at low pressure.
(ii) Interpret the behaviour of real gas with respect to ideal gas at high pressure.
(iii) Mark the pressure and volume by drawing a line at the point where real gas behaves as an ideal gas.
(i) At low pressure, the real gas shows very small deviation from ideal behaviour because the two curves almost coincide at low pressure.
(ii) At high pressure, the real gas show large deviations from ideal behaviour as the curves are far apart.
(iii) At point ' $A$ ', both the curves intersect each other. At this point real gas behaves as an ideal gas. $p_1$ and $V_1$ are the pressure and volume which corresponds to this point $A$.
Match the graphs between the following variables with their names.
| Graphs | Names | ||
|---|---|---|---|
| A. | Pressure vs temperature graph at constant molar volume | 1. | Isotherms |
| B. | Pressure vs volume graph at constant temperature | 2. | Constant temperature curve |
| C. | Volume vs temperature graph at constant pressure | 3. | Isochores |
| 4. | Isobars |
$$\mathrm{A.\to(3)\quad \mathrm{B.} \to (1)\quad \mathrm{C.}\to(4)}$$
A. When molar volume is constant, the $p-T$ graph is called isochore.
B. When temperature is constant, the $p-V$ graph is called isotherm.
C. When pressure is constant, $V-T$ graph is called isobar.
Match the following gas laws with the equation representing them.
| Graphs | Names | ||
|---|---|---|---|
| A. | Boyle's law | 1. | $V \propto n$ at constant $T$ and $p$ |
| B. | Charle's law | 2. | $p_{\text {Total }}=p_1+p_2+p_3+\ldots$ at constant $T, V$ |
| C. | Dalton's law | 3. | $\frac{p V}{T}=$ constant |
| D. | Avogadro's law | 4. | $V \propto T$ at constant $n$ and $p$ |
| 5. | $p \propto \frac{1}{V}$ at constant $n$ and $T$ |
A. $\rightarrow(5)$
B. $\rightarrow(4)$
C. $\rightarrow(2)$
D. $\rightarrow$ (1)
A. Boyle's law, $p \propto \frac{1}{V}$ at constant $T$ and $n$.
B. Charle's law, $V \propto T$ at constant $p$ and $n$.
C. Dalton's law, $p_{\text {Total }}=p_1+p_2+p_3+\ldots$ at constant $T, V$.
D. Avogadro's law, $V \propto n$ at constant $T$ and $p$.