If 4 moles of hydrogen gas react with excess oxygen, how many moles of water are produced?

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Multiple Choice

If 4 moles of hydrogen gas react with excess oxygen, how many moles of water are produced?

Explanation:
In combustion-style stoichiometry, the amounts of reactants and products relate directly through the balanced equation. For hydrogen reacting with oxygen, the balanced form is 2 H2 + O2 -> 2 H2O, which shows a 1:1 relationship between H2 and H2O (both have a coefficient of 2). Since oxygen is in excess, hydrogen is the limiting reagent, so the moles of water produced equal the moles of hydrogen consumed. With 4 moles of H2, the calculation is 4 moles H2 × (2 moles H2O / 2 moles H2) = 4 moles H2O. Therefore, four moles of water are produced.

In combustion-style stoichiometry, the amounts of reactants and products relate directly through the balanced equation. For hydrogen reacting with oxygen, the balanced form is 2 H2 + O2 -> 2 H2O, which shows a 1:1 relationship between H2 and H2O (both have a coefficient of 2). Since oxygen is in excess, hydrogen is the limiting reagent, so the moles of water produced equal the moles of hydrogen consumed. With 4 moles of H2, the calculation is 4 moles H2 × (2 moles H2O / 2 moles H2) = 4 moles H2O. Therefore, four moles of water are produced.

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