1. Kinetic Theory, Temperature, and Pressure
Temperature is a measure of the average translational kinetic energy of a system's particles; gas pressure is the aggregate result of countless particle collisions with a container's walls.
Average kinetic energy per particle: $KE_avg=/32k_BT$ (T in kelvin only), with $k_B=1.38×10^-23$ J/K. RMS speed: $v_rms=sqrt/3k_BTm=sqrt/3RTM$.
Temperature (average KE per particle, intensive, independent of amount) vs. internal/thermal energy (total KE of all particles, extensive) --- doubling the amount of gas at the same T doubles internal energy but does NOT change temperature.
Plugging a Celsius temperature directly into $KE_avg=/32k_BT$ or any gas law --- always convert to kelvin ($T_K=T_C+273$) before using any kinetic-theory or gas-law formula.
$KE_avg=/32k_BT$, always kelvin; higher T means faster average molecular speed, not more particles.