Question:Dalton’s law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of gases making up the mixture. Give a convincing argument for this law based on the kinetic theory of gases. Answer to this question from the book I study Physics gives an explanation stating molecules of different kinds collide with the wall of the container so each additional number of molecules add an extra pressure to the total. But it doesn't say anything about Temperature. How about the second gas you mix with the first has 4 times the number of molecules of first but has temperature of near oK, say 50K? wouldn't than the total pressure be LESS than initial one as the new bunch of molecules' kinetic energy will slow down the total molecules' and the pressure will go down?