Use one assumption of the kinetic theory of gases to explain why the molecules of an ideal gas have zero potential energy.
The mean translational kinetic energy $E_{K}$ of one molecule of an ideal gas is written as $E_{K} = \frac{1}{2} m\langle c^{2} \rangle = \frac{3}{2}kT$, where $m$ is the mass of a molecule and $k$ is the Boltzmann constant. State what the symbol $\langle c^{2} \rangle$ means.
State the meaning of $T$ in the expression $E_{K} = \frac{1}{2} m\langle c^{2} \rangle = \frac{3}{2}kT$.
An iron cylinder of fixed volume $4.7 \times 10^{4}\,\text{cm}^{3}$ contains an ideal gas at pressure $2.6 \times 10^{5}\,\text{Pa}$ and temperature $173^{\circ}\text{C}$. The gas is heated, and $2900\,\text{J}$ of thermal energy is transferred to it. Calculate the number $N$ of molecules in the cylinder.
Calculate the rise in average kinetic energy of one molecule during the heating process.
Use your answer in part (c)(i).2 to determine the final temperature $T$, in kelvin, of the gas in the cylinder.
Find the increase in average kinetic energy of one molecule during the heating process.
Use your answer in (i) part 2 to determine the final temperature $T$, in kelvin, of the gas in the cylinder.