At absolute zero temperature, pressure of a gas will be
A
Zero
B
One atmospheric pressure
C${P_0} \times 273$
D${P_0} \times 76$
Easy
Download our app for free and get started
A
Zero
a $PV = \mu RT,$ $T = 0,$
$\therefore \,\,P = 0$ Because $V \ne 0$
Download our app
and get started for free
Experience the future of education. Simply download our apps or reach out to us for more information. Let's shape the future of learning together!No signup needed.*
You have two containers of equal volume. One is full of helium gas. The other holds an equal mass of nitrogen gas. Both gases have the same pressure. How does the temperature of the helium compare to the temperature of the nitrogen ?
Gas at a pressure ${P_0}$ in contained is a vessel. If the masses of all the molecules are halved and their speeds are doubled, the resulting pressure $P$ will be equal to
The figure shows the volume $V$ versus temperature $T$ graphs for a certain mass of a perfect gas at two constant pressures of ${P_1}$ and ${P_2}$. What interference can you draw from the graphs
Consider a mixture of $n$ moles of helium gas and $2 n$ moles of oxygen gas (molecules taken to be rigid) as an ideal gas. Its $\frac{\mathrm{C}_{\mathrm{P}}}{\mathrm{C}_{\mathrm{V}}}$ value will be
A gas is filled in a vessel at a pressure given by $P = \left( {6.02 \times {{10}^{23}}} \right)kT$ where $k$ is the Boltzmann constant and $T$ is the absolute temperature. The number of molecules per unit volume of the gas is