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

Question

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

Serenity Allen · Accepted Answer

5.9 g of hydrogen must react.

1. Write the equation that is balanced. #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#

Natalie Anton · Answer

undefined To find the grams of hydrogen that reacted, you can use stoichiometry and the given equation. First, calculate the molar mass of oxygen (O2), which is 2 * 16.00 g/mol = 32.00 g/mol. Then, use the stoichiometric coefficients from the equation to find the molar ratio of hydrogen to oxygen: 2 mol of H2 for every 1 mol of O2. Finally, set up a proportion to find the grams of hydrogen: (47 g O2) * (2 mol H2 / 1 mol O2) * (2.02 g/mol H2) = approximately 190 g of hydrogen.

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

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