**Stoichiometry Problem: Sulfur Reaction with Nitric Acid**Consider the following balanced chemical equation:\[ \text{S} + 6 \text{HNO}_3 \rightarrow \text{H}_2\text{SO}_4 + 6 \text{NO}_2 + 2 \text{H}_2\text{O} \]The problem to solve is:**Question:** In the above equation, how many moles of \( \text{H}_2\text{SO}_4 \) can be made when 46 moles of \( \text{HNO}_3 \) are consumed?**Solution Explanation:**1. **Identify the Mole Ratio:** From the balanced chemical equation, we see that the mole ratio between \( \text{HNO}_3 \) and \( \text{H}_2\text{SO}_4 \) is 6:1. This means that for every 6 moles of \( \text{HNO}_3 \) consumed, 1 mole of \( \text{H}_2\text{SO}_4 \) is produced.2. **Calculate the Moles of \( \text{H}_2\text{SO}_4 \):** We are given 46 moles of \( \text{HNO}_3 \). To find out how many moles of \( \text{H}_2\text{SO}_4 \) are produced, we use the mole ratio from the balanced equation.\[ \frac{46 \text{ moles } \text{HNO}_3}{6} = \text{7.67 moles of } \text{H}_2\text{SO}_4 \]Therefore, 7.67 moles of \( \text{H}_2\text{SO}_4 \) can be made when 46 moles of \( \text{HNO}_3 \) are consumed.

given, moles of HNO3 = 46 moles

Answered: S + 6 HNO3 --> H₂SO4 + 6 NO2 + 2H₂O In…

S + 6 HNO3 --> H₂SO4 + 6 NO2 + 2H₂O In the above equation how many moles of H₂SO4 can be made when 46 moles of HNO3 are consumed?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

**Stoichiometry Problem: Sulfur Reaction with Nitric Acid**

Consider the following balanced chemical equation:

\[ \text{S} + 6 \text{HNO}_3 \rightarrow \text{H}_2\text{SO}_4 + 6 \text{NO}_2 + 2 \text{H}_2\text{O} \]

The problem to solve is:

**Question:** In the above equation, how many moles of \( \text{H}_2\text{SO}_4 \) can be made when 46 moles of \( \text{HNO}_3 \) are consumed?

**Solution Explanation:**

1. **Identify the Mole Ratio:**
From the balanced chemical equation, we see that the mole ratio between \( \text{HNO}_3 \) and \( \text{H}_2\text{SO}_4 \) is 6:1. This means that for every 6 moles of \( \text{HNO}_3 \) consumed, 1 mole of \( \text{H}_2\text{SO}_4 \) is produced.

2. **Calculate the Moles of \( \text{H}_2\text{SO}_4 \):**
We are given 46 moles of \( \text{HNO}_3 \). To find out how many moles of \( \text{H}_2\text{SO}_4 \) are produced, we use the mole ratio from the balanced equation.

\[ \frac{46 \text{ moles } \text{HNO}_3}{6} = \text{7.67 moles of } \text{H}_2\text{SO}_4 \]

Therefore, 7.67 moles of \( \text{H}_2\text{SO}_4 \) can be made when 46 moles of \( \text{HNO}_3 \) are consumed.

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