1. The problem statement, all variables and given/known data The total pressure of a mixture of oxygen and hydrogen is 1.00 atm. The mixture is ignited and the water produced is removed. The remaining gas is pure hydrogen and exerts a pressure of 0.34 atm when measured in the same volume and at the same temperature as the original mixture. What was the composition of the original mixture in mole percent? 2. Relevant equations 2H2 +O2 ---> 2H2O 3. The attempt at a solution 1atm - 0.34atm = 0.66atm H2O for every 1 mol of H2 that reacts, 2 mols of H2 react so, 0.44atm of the water is H2 0.22 atm of the water is O2 0.34atm +0.44atm = 0.78atm H2O 0.22atm O2 78% of the mixture is H2 22% of the mixture is O2 Can someone check this?