Molar specific heat of oxygen at constant pressure ${\mathrm{C}}_{\mathrm{P}}=7.2 \mathrm{cal}/\mathrm{mol}°\mathrm{C} \mathrm{and} \mathrm{R}=8.3 \mathrm{joule}/\mathrm{mol}/\mathrm{K}.$ At constant volume, 5 mol of oxygen is heated from $10°\mathrm{C} \mathrm{to} 20°\mathrm{C},$ the quantity of heat required is approximately

1.  $25 \mathrm{cal}$                               

2.  $50 \mathrm{cal}$

3.  $250 \mathrm{cal}$                             

4.  $500 \mathrm{cal}$

One mole of an ideal gas requires 207 J heat to raise the temperature by 10 K when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by the same 10 K, the heat required is

1.  198.7 J                 

2.  29 J

3.  215.3 J                 

4.  124 J

(Given the gas constant $\mathrm{R}=8.3 \mathrm{J}/\mathrm{mol}‐\mathrm{K}$)

The expansion of an ideal gas of mass m at a constant pressure P is given by the straight line D. Then the expansion of the same ideal gas of mass 2m at a pressure P/ 2 is given by the straight line , where number on graphs indicate slope , is- 

1.  E                           

2.  C

3.  B                           

4.  A

An experiment is carried out on a fixed amount of gas at different temperatures and at high pressure such that it deviates from the ideal gas behaviour. The variation of $\frac{\mathrm{PV}}{\mathrm{RT}}$ with P is shown in the diagram. The correct variation will correspond to: (Assuming that the gas in consideration is nitrogen)

The figure below shows the graph of pressure and volume of a gas at two temperatures \(T_1\) and \(T_2.\) Which one, of the following, inferences is correct?

The expansion of unit mass of a perfect gas at constant pressure is shown in the diagram. Here

1. a = volume, b = $°\mathrm{C}$ temperature

2. a = volume, b = $\mathrm{K}$ temperature

3. a = $°\mathrm{C}$ temperature, b = volume

4. a = $\mathrm{K}$ temperature, b = volume

An ideal gas is initially at temperature T and volume V. Its volume increases by $∆\mathrm{V}$ due to an increase in temperature $∆\mathrm{T}$, pressure remaining constant. The quantity $\mathrm{\delta }=∆\mathrm{V}/\left(\mathrm{V}∆\mathrm{T}\right)$ varies with temperature as:

1.		2.
3.		4.

Pressure versus temperature graph of an ideal gas of equal number of moles of different volumes are plotted as shown in figure. Choose the correct alternative

1. ${\mathrm{V}}_1={\mathrm{V}}_2 , {\mathrm{V}}_3={\mathrm{V}}_4 \mathrm{and} {\mathrm{V}}_2>{\mathrm{V}}_3$

2. ${\mathrm{V}}_1={\mathrm{V}}_2 , {\mathrm{V}}_3={\mathrm{V}}_4 \mathrm{and} {\mathrm{V}}_2<{\mathrm{V}}_3$

3. ${\mathrm{V}}_1={\mathrm{V}}_2 , {\mathrm{V}}_3={\mathrm{V}}_4$

4. ${\mathrm{V}}_4>{\mathrm{V}}_3 > {\mathrm{V}}_2>{\mathrm{V}}_1$

Pressure versus temperature graph of an ideal gas is as shown in figure. Density of the gas at point A is ${\mathrm{\rho }}_0$ . Density at B will be

1.  $\frac{3}{4}{\mathrm{\rho }}_0$                             

2.  $\frac{3}{2}{\mathrm{\rho }}_0$

3.  $\frac{4}{3}{\mathrm{\rho }}_0$                             

4.  $2 {\mathrm{\rho }}_0$

Graph of specific heat at constant volume for a monoatomic gas is

1.                          

2. 

3.                        

4.