The balanced chemical equation for the reaction of hydrogen and oxygen is shown below.
[tex]2 H_2+O_2 \rightarrow 2 H_2 O[/tex]
The number of moles of hydrogen that is needed to produce 0.253 mol of water is
A. smaller than 0.253 mol.
B. much greater than 0.253 mol.
C. slightly greater than 0.253 mol.
D. equal to 0.253 mol.
Answer (2)
In this reaction, the molar ratio between hydrogen and water is 1:1. Therefore, to produce 0.253 mol of water, 0.253 mol of hydrogen is needed. The correct answer is D. equal to 0.253 mol.
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The balanced chemical equation shows a 1:1 molar ratio between hydrogen and water.
Calculate the moles of hydrogen needed: 0.253 mol H 2 O × 2 mol H 2 O 2 mol H 2 = 0.253 mol H 2 .
Compare the calculated moles of hydrogen with 0.253 mol.
The number of moles of hydrogen needed is equal to 0.253 mol, so the answer is equal to 0.253 mol .
Explanation
Understanding the Problem We are given the balanced chemical equation for the reaction of hydrogen and oxygen to produce water: 2 H 2 + O 2 i g h t ha r p oo n u p 2 H 2 O We are asked to determine the number of moles of hydrogen needed to produce 0.253 mol of water and compare it to 0.253 mol.
Determining the Molar Ratio From the balanced chemical equation, we can see that 2 moles of hydrogen ( H 2 ) react to produce 2 moles of water ( H 2 O ). This means the molar ratio between hydrogen and water is 2:2, which simplifies to 1:1.
Calculating Moles of Hydrogen To calculate the moles of hydrogen required to produce 0.253 mol of water, we use the molar ratio: Moles of H 2 = (Moles of H 2 O ) * (Coefficient of H 2 / Coefficient of H 2 O )
Moles of H 2 = (0.253 mol) * (2 / 2) Moles of H 2 = 0.253 mol * 1 Moles of H 2 = 0.253 mol
Comparison and Conclusion Now we compare the calculated moles of hydrogen (0.253 mol) with 0.253 mol. Since they are equal, the number of moles of hydrogen needed to produce 0.253 mol of water is equal to 0.253 mol.
Examples
In the Haber-Bosch process, nitrogen and hydrogen react to produce ammonia, a crucial component of fertilizers. Understanding the stoichiometry of this reaction allows us to calculate the exact amounts of hydrogen needed to react with a given amount of nitrogen to maximize ammonia production. This ensures efficient use of resources and minimizes waste, which is vital in industrial chemical processes. By applying stoichiometric principles, chemical engineers can optimize reaction conditions and improve the yield of desired products, contributing to sustainable and cost-effective manufacturing.
