For three low density gases \(A , B , C\) pressure versus temperature graphs are plotted while keeping them at constant volume, as shown in the figure.The temperature corresponding to the point ' \(K\) ' is :
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For isochoric processes, the ratio of pressure to temperature is constant. Remember to convert Celsius to Kelvin when dealing with gas laws.
The given question requires understanding the behavior of low-density gases under constant volume conditions, which is typically described by the ideal gas law.
According to the ideal gas law, for a given amount of gas at constant volume, the pressure \( P \) is directly proportional to its absolute temperature \( T \) (in Kelvin). The relationship is given by:
P \propto T
This implies that the pressure-temperature graph should extrapolate to the origin at absolute zero temperature.
The graph shown in the question depicts the pressure vs. temperature plot for three gases \( A, B, \) and \( C \). The point \( K \) where the plot intersects the temperature axis is the point where the pressure is zero.
This point is crucial because it represents absolute zero temperature in Celsius. Absolute zero is the theoretical lowest temperature possible and is equivalent to:
0 \, \text{K} = -273.15^{\circ} \text{C}
As such, the temperature corresponding to the point \( K \) is approximately:
