Using the equation #2H_2 + O_2 -> 2H_2O#, when 47g of oxygen are produced, how many grams of hydrogen must react?

1 Answer
Jul 2, 2016

Answer:

5.9 g of hydrogen must react.

Explanation:

1. Write the balanced equation.

#2"H"_2 + "O"_2 → "2H"_2"O"#

2. Calculate the moles of #"O"_2#.

#"Moles of O"_2 = 47 color(red)(cancel(color(black)("g O"_2))) × ("1 mol O"_2)/(32.00 color(red)(cancel(color(black)("g O"_2)))) = "1.47 mol O"_2#

3. Calculate the moles of #"H"_2#.

#"Moles of H"_2 = 1.47 color(red)(cancel(color(black)("mol O"_2))) × ("2 mol H"_2)/(1 color(red)(cancel(color(black)("mol O"_2)))) = "2.94 mol H"_2#

4. Calculate the mass of #"H"_2#.

#"Mass of H"_2 = 2.94 color(red)(cancel(color(black)("mol H"_2))) × ("2.016 g H"_2)/(1 color(red)(cancel(color(black)("mol H"_2)))) = "5.9 g H"_2#