A gas at 300 K has pressure `4 xx 10^(-10) N//m^(2)`. IF `k = 1.38 xx 10^(-23) J//K`, the number of `"molecule"// cm^(3)` is of the order of

A gas is at temperature 80^(@)C and pressure 5xx10^(-10)Nm^(-2) . What is the number of molecules per m^(3) if Boltzmann's constant is 1.38xx10^(-23)JK^(-1)

The molar specific heat of an ideal gas at constant pressure is C_(p) = 5/2 R . Some amount of this gas in a closed container has a volume 0.0083 m^(3) , a temperature 300 K and a pressure 1.6 xx 10^(6) N cdot m^(-2) . If 2.49 xx 10^(4) J 1 of heat is supplied at a constant volume of the gas, find out the final temperature and pressure. Given, R = 8.3 J cdot mol^(-1) cdot K^(-1) .

Calculate the KE per molecule and also rms velocity of a gas at 127^(@)C . Given k = 1.38 xx 10^(-23) J "molecule"^(-1) K^(-1) and mass of each molecule = 6.4 xx 10^(-27) kg .

The number of gas molecules striking per second per square meter of the top surface of a table placed in a room at 20^(@)C and 1 atmospheric pressure is of the order of (k_(B) = 1.4 xx10^(-23) J/K, and the average mass of an air molecules is 5xx10^(-27) kg)