Answer: 32g of oxygen and 4g of hydrogen were reacted in total.
Step-by-step explanation:
To find out how many grams of reactants were reacted, we need to use the balanced equation of the reaction. The equation for the reaction between hydrogen and oxygen to produce hydrogen peroxide is:
2H2 + O2 --> 2H2O2
From the equation, we know that the reaction involves 2 moles of hydrogen and 1 mole of oxygen. We can use the balanced equation to determine the stoichiometry of the reaction, which tells us the relative number of moles of each reactant and product.
We know that 32g of oxygen was reacted, and since 1 mole of oxygen is equal to 16g, we can calculate the number of moles of oxygen by:
32g / 16g = 2 moles
We know that 2 moles of hydrogen are required for every mole of oxygen. so the number of moles of hydrogen is also 2 moles.
We know that 1 mole of hydrogen is equal to 2g, so we can calculate the number of grams of hydrogen by:
2 moles x 2g = 4g
Therefore, 32g of oxygen and 4g of hydrogen were reacted in total.