2H2O2 → 2H2O + O2 How many moles of hydrogen peroxide (H2O2) are needed to produce 5.0 moles of water? 10 moles
The Correct Answer and Explanation is:
To determine how many moles of hydrogen peroxide (H2O2) are required to produce 5.0 moles of water (H2O), we need to analyze the balanced chemical equation:
2H2O2 → 2H2O + O2
From the equation, we observe the following mole ratio:
- For every 2 moles of hydrogen peroxide (H2O2), 2 moles of water (H2O) are produced.
This implies that the moles of H2O2 and H2O are in a 1:1 ratio. Therefore, the number of moles of hydrogen peroxide needed is equal to the number of moles of water produced.
If we are given that 5.0 moles of water are produced, then the moles of hydrogen peroxide required will also be:
5.0 moles of H2O2
Step-by-Step Breakdown:
- Balanced Chemical Equation:
2H2O2→2H2O+O22H2O2 → 2H2O + O22H2O2→2H2O+O2 - Mole Ratio Analysis:
- From the equation, the ratio of H2O2 to H2O is 1:1. This means 1 mole of H2O2 produces 1 mole of H2O.
- Given Information:
- You are given that 5.0 moles of water (H2O) are produced.
- Calculate the Required Moles of H2O2:
- Since the ratio is 1:1, 5.0 moles of water will be produced from 5.0 moles of hydrogen peroxide.
Thus, 5.0 moles of hydrogen peroxide are needed to produce 5.0 moles of water.
Explanation:
The balanced chemical equation tells us the exact stoichiometric relationship between the reactants and products. Because the number of moles of H2O2 required is the same as the number of moles of H2O produced, this simplifies the calculation significantly, making it a straightforward 1:1 conversion. The mole-to-mole ratio directly gives us the number of moles needed for the reaction.
