Use the following balanced equation for problems 1–5. Molar masses are given below. 2 As + 3 H2 2 AsH3 + 150. kcal molar masses 74.92 g 2.02 g 77.95 g How many moles of hydrogen are required to react with 25.00 moles of arsenic, As ?
Use the following balanced equation for problems 1–5. Molar masses are given below. 2 As + 3 H2 2 AsH3 + 150. kcal molar masses 74.92 g 2.02 g 77.95 g How many moles of hydrogen are required to react with 25.00 moles of arsenic, As ?
Biochemistry
9th Edition
ISBN:9781319114671
Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Chapter1: Biochemistry: An Evolving Science
Section: Chapter Questions
Problem 1P
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![Use the following balanced equation for problems 1-5. Molar masses are given below.
\[
2 \text{As} + 3 \text{H}_2 \rightarrow 2 \text{AsH}_3 + 150. \text{kcal}
\]
Molar masses:
- As: 74.92 g
- H₂: 2.02 g
- AsH₃: 77.95 g
**Question:**
How many moles of hydrogen are required to react with 25.00 moles of arsenic, As?
- A. 75.00 mol
- B. 25.00 mol
- C. 16.67 mol
- D. 37.50 mol
**Explanation:**
To solve, use the stoichiometry from the balanced equation. Based on the equation, to react 2 moles of As, 3 moles of H₂ are needed. Thus, for 25.00 moles of As:
\[
\left(\frac{3 \text{ moles of } \text{H}_2}{2 \text{ moles of As}} \right) \times 25.00 \text{ moles of As} = 37.50 \text{ moles of } \text{H}_2
\]
Therefore, the correct answer is **D. 37.50 mol**.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3af619a8-05d7-4a08-b6ab-836abf944ec6%2Ff8713ece-6629-4002-bf70-af3643fd4f5e%2Fwixfdfv_processed.png&w=3840&q=75)
Transcribed Image Text:Use the following balanced equation for problems 1-5. Molar masses are given below.
\[
2 \text{As} + 3 \text{H}_2 \rightarrow 2 \text{AsH}_3 + 150. \text{kcal}
\]
Molar masses:
- As: 74.92 g
- H₂: 2.02 g
- AsH₃: 77.95 g
**Question:**
How many moles of hydrogen are required to react with 25.00 moles of arsenic, As?
- A. 75.00 mol
- B. 25.00 mol
- C. 16.67 mol
- D. 37.50 mol
**Explanation:**
To solve, use the stoichiometry from the balanced equation. Based on the equation, to react 2 moles of As, 3 moles of H₂ are needed. Thus, for 25.00 moles of As:
\[
\left(\frac{3 \text{ moles of } \text{H}_2}{2 \text{ moles of As}} \right) \times 25.00 \text{ moles of As} = 37.50 \text{ moles of } \text{H}_2
\]
Therefore, the correct answer is **D. 37.50 mol**.
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