Two vessels A and B contain same mass of Oxygen and Hydrogen respectively at the same temperature. The volume of B is twice that of A. The ratio of gas pressure in A to that in B is

Step-by-step solution

Using the ideal gas equation, PV = nRT = m M RT , where m is the given mass and M is the molar mass. For vessel A containing Oxygen ( O₂ , M_A = 32 ): P_A = mRT 32 V_A For vessel B containing Hydrogen ( H₂ , M_B = 2 ): P_B = mRT 2 V_B Given that the volume of B is twice that of A ( V_B = 2V_A ), we get: P_B = mRT 2(2V_A) = mRT 4V_A Taking the ratio of the pressures: P_A P_B = mRT 32 V_A mRT 4 V_A = 4 32 = 1 8 The ratio of gas pressure in A to that in B is 1:8 . Answer: 1:8