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**.

The stoichiometric relation in the reaction says that 2 moles of arsenic (As) is required to react…

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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 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 ?