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

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Answer 1 · 2016-07-02T22:19:37

5.9 g of hydrogen must react.

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 $"H"_2$ .

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

Using the equation 2H_2 + O_2 -> 2H_2O2H_2 + O_2 -> 2H_2O, when 47g of oxygen are produced, how many grams of hydrogen must react?