Show that the molar volume of an ideal gas at STP is 22.4 litres. Given `R=8.31 Jmol^(-1) K^(-1)`.

Three moles of an ideal gas at a constant temperature of 300 K is compressed from a volume of 4 litres to 1 litre. Calculate the work done in the process. Given R=8.31 Jmol^-1K^-1 .

The mass of 16.4 dm^3 of a gas at STP is 22g. What is the molar mass of the gas?

The rate constants of a reaction at 500K and 700K are 0.02s^-1 and 0.07s^-1 respectively. Calculate value of activation energy for the reaction. (Given R = 8.314 JK^-1 mol^-1)

Prove that the pressure exerted by an ideal gas given by P=1/3 rhov^2 .

The rate constant of reaction is 1.5xx10^7s^-1 at 50^@C and 4.5xx10^7s^-1 at 100^@C . Calculate the value of activation energy for the energy for the reaction (R = 8.314 Jk^-1 mol^-1)

With the help of Avogadro's hypothesis prove that the molar volume of all gases is 22.4 dm^3 at STP.

What is the density of SO_2 gas at 27^@C at 2 atmospheric pressure?(R = 0.08219 atm K^(-1) mol^(-1)

For a decomposition reaction, the values of rate constants at two different temperatures are given below: K_1 = 2.15xx10^-8 Lmol^-1s^-1 at 650k K_2 = 2.39xx10^-7 Lmol^-1s^-1 at 700k Calculate the value of activation energy for the reaction (R = 8.314 JK^-1 mol^-1 )

The rate of reaction triples when temperature change from 20^@C to 50^@C . Calculate the energy of activation. (R = 8.314 Jmol^-1K^-1)

The rate constant of a reaction at 500K and 700K are 0.01s^-1 and 0.07s^-1 respectively. Calculate the value of activation energy for the reaction (R = 8.314 JK^-1mol^-1).