For V versus T curves at constant pressure `P_1 and P_2` for and ideal gas shown in figure-

V vs T curves at constant pressure P_(1) and P_(2) for an ideal gas are shown below Which is correct ?

V vs T curves at different pressures P_(1) and P_(2) for an ideal gas are shown below: Which one of the following is correct?

For an ideal gas V - T curves at constant pressure P_(1) & P_(2) are shown in figure, from the figure

Pressure versus density graph of an ideal gas is shown in figure

A plot of P vs T for a given mass of gas at constant volume is a straight line . P vs T at constant volumes V_(1) and V_(2) for an ideal gas are shown below : Which of the following is correct ?

For one mole of an ideal gas the slope of V versus T curve at constant pressure of 2 atm is X lit mol^(-1) K^(-1) . The value of the ideal universal gas constant 'R' in terms of X is "___________" .

One mole of an ideal monatomic gas undergoes a linear process from A to B , in which is pressure P and its volume V change as shown in figure . The absolute temperature T versus volume V for the given process is

The volume V versus temperature T graphs for a cetain amount of a perfect gas at two pressure p_1 and p_2 are as shown in Fig. It follows from the graphs that p_1 is greater than p_2.

Volume versus temperature graphs for a given mass of an ideal gas are shown in figure. At two different values of constant pressure. What can be inferred about relation between P_(1) and P_(2) ?