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+T=273;//temperature 0C in kelvin//
+R=8.31*10^7;//Universal gas constant in erg per degree per mole//
+M=28;//molecular weight of N2 in gram per mole//
+printf('Since 22.4Litres of Nitrogen gas at 0C and 1atm pressure will contain 6.023*10^23Molecules.');
+N=2.69*10^19;//no. of molecules in molecules per cm^3//
+G=3.78*10^-8;//collision diameter in cm//
+K=sqrt(%pi*R*T/M);
+Z11=2*N^2*G^2*K;//number of collisions per second of Nitrogen at 0C and 1atm//
+printf('\nNumber of molecular collisions per second of Nitrogen at 0C and 1atm=%f=10.43*10^28molecular collisions per sec per cm^3',Z11);