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How many moles of BeCl2 are needed to react completely with 1.75 moles of LiH?

How many moles of BeCl2 are needed to react completely with 1.75 moles of LiH?

Chemistry
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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**Question:** How many moles of BeCl₂ are needed to react completely with 1.75 moles of LiH? **Explanation and Approach:** To answer this question, we need to look at the balanced chemical equation for the reaction between beryllium chloride (BeCl₂) and lithium hydride (LiH). The typical reaction can be represented as: \[ \text{BeCl}_2 + \text{2LiH} \rightarrow \text{BeH}_2 + \text{2LiCl} \] From the balanced equation, you can observe the molar ratio between BeCl₂ and LiH is 1:2. This means that 1 mole of BeCl₂ reacts with 2 moles of LiH. To find out how many moles of BeCl₂ are needed to react completely with 1.75 moles of LiH, we can use this stoichiometric ratio. We'll set up a proportion based on the ratio: \[ \text{Moles of BeCl}_2 = \frac{1 \text{ mole of BeCl}_2}{2 \text{ moles of LiH}} \times 1.75 \text{ moles of LiH} \] \[ \text{Moles of BeCl}_2 = \frac{1}{2} \times 1.75 \] \[ \text{Moles of BeCl}_2 = 0.875 \] **Conclusion:** 0.875 moles of BeCl₂ are needed to react completely with 1.75 moles of LiH.
Transcribed Image Text:**Question:** How many moles of BeCl₂ are needed to react completely with 1.75 moles of LiH? **Explanation and Approach:** To answer this question, we need to look at the balanced chemical equation for the reaction between beryllium chloride (BeCl₂) and lithium hydride (LiH). The typical reaction can be represented as: \[ \text{BeCl}_2 + \text{2LiH} \rightarrow \text{BeH}_2 + \text{2LiCl} \] From the balanced equation, you can observe the molar ratio between BeCl₂ and LiH is 1:2. This means that 1 mole of BeCl₂ reacts with 2 moles of LiH. To find out how many moles of BeCl₂ are needed to react completely with 1.75 moles of LiH, we can use this stoichiometric ratio. We'll set up a proportion based on the ratio: \[ \text{Moles of BeCl}_2 = \frac{1 \text{ mole of BeCl}_2}{2 \text{ moles of LiH}} \times 1.75 \text{ moles of LiH} \] \[ \text{Moles of BeCl}_2 = \frac{1}{2} \times 1.75 \] \[ \text{Moles of BeCl}_2 = 0.875 \] **Conclusion:** 0.875 moles of BeCl₂ are needed to react completely with 1.75 moles of LiH.
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