4g of Hydrogen reacts with 50g of oxygen. 1. How much oxygen is used ? 2. What is the amount of water? Share with your friends Share 0 Goutam Pradhan answered this Dear Student, The balanced equation is2H2 + O2→2H2OWe are given 4g H2 = 4g2 g/mol= 2moland 50g O2 = 50g32 g/mol=1.5625 molAccording to balanced equation 2 mol H2 reacts with 1 mol O2But we have 1.5625 mol O2, so H2 is limiting reagent(i) This means 0.5625 mol O2 will be left behind= 0.5625 mol x 32 g/mol =18 g(ii) 2 mol H2 produces 2 mol H2O =2 mol x 18 g/mol = 36g Regards 1 View Full Answer Pratyush answered this Correct option isC 22.5g H2+21O2⟶H2O Mass-4g20g Moles-20.625 1 mole of H2 requires 0.5 moles of O2. ∴ 1.25 moles of H2 requires 0.625 moles of O2 ∴ O2 is a limiting reagent. 0.5 mole O2⟶1 mole H2O ∴0.625 mole O2=0.51×0.625 moles H2O. =1.25 moles of H2O Therefore, mass of H2O formed =1.25×18=22.5 gm Hence, option C is correct. 0