A hydrogen-filled balloon was ignited and 1.70 g of hydrogen reacted with 13.6 g of oxygen. How much water vapor is formed assuming only water vapor is formed
Can you please explain how it’s done also. This is the only question I’ve had trouble with on my homework assignment for next week.
2 H2 + O2 = 2 H2O
moles H2 = 1.70/ 2.016=0.843
moles O2 = 13.6/32 g/mol=0.425
H2 is the limiting reactant : 0.425 x 2 = 0.850 moles of H2 are needed
moles H2O = 0.843
mass H2O = 0.843 x 18.02 g/mol= 15.2 g