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How many moles of BCl3 are needed to produce 5.00 g of HCl(aq) in the following reaction? BCl3(g) + 3 H₂O(l) → 3 HCl(aq) + B(OH)3(aq)

How many moles of BCl3 are needed to produce 5.00 g of HCl(aq) in the following reaction? BCl3(g) + 3 H₂O(l) → 3 HCl(aq) + B(OH)3(aq)

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Could I have with the following two problems, I am confused and I  just need to analyze the work on how to solve tese two problem

**Chemical Reaction Problem: How Many Moles of BCl₃ are Required?** **Scenario:** Calculate the number of moles of BCl₃ needed to produce 5.00 g of HCl(aq) in the following chemical reaction: \[ \text{BCl}_3(g) + 3 \text{H}_2\text{O}(l) \rightarrow 3 \text{HCl}(aq) + \text{B(OH)}_3(aq) \] **Understanding the Reaction:** - **Reactants:** Boron trichloride (BCl₃) and water (H₂O). - **Products:** Hydrochloric acid (HCl) and boric acid (B(OH)₃). The balanced equation shows a 1:3 molar ratio between BCl₃ and HCl, indicating that 1 mole of BCl₃ produces 3 moles of HCl. To solve the problem, calculate the moles of HCl produced from 5.00 g and then determine the corresponding moles of BCl₃ required.
Transcribed Image Text:**Chemical Reaction Problem: How Many Moles of BCl₃ are Required?** **Scenario:** Calculate the number of moles of BCl₃ needed to produce 5.00 g of HCl(aq) in the following chemical reaction: \[ \text{BCl}_3(g) + 3 \text{H}_2\text{O}(l) \rightarrow 3 \text{HCl}(aq) + \text{B(OH)}_3(aq) \] **Understanding the Reaction:** - **Reactants:** Boron trichloride (BCl₃) and water (H₂O). - **Products:** Hydrochloric acid (HCl) and boric acid (B(OH)₃). The balanced equation shows a 1:3 molar ratio between BCl₃ and HCl, indicating that 1 mole of BCl₃ produces 3 moles of HCl. To solve the problem, calculate the moles of HCl produced from 5.00 g and then determine the corresponding moles of BCl₃ required.
### Extraction of Iron from Iron Ore Mining companies extract iron from iron ore according to the following balanced chemical equation: \[ \text{Fe}_2\text{O}_3(s) + 3\text{CO}(g) \rightarrow 2\text{Fe}(s) + 3\text{CO}_2(g) \] In a reaction mixture containing 169 g of \(\text{Fe}_2\text{O}_3\) and 73.8 g of CO, CO is the limiting reactant. #### Part A Calculate the mass of the reactant in excess (which is \(\text{Fe}_2\text{O}_3\)) that remains after the reaction has gone to completion. Express the mass with the appropriate units.
Transcribed Image Text:### Extraction of Iron from Iron Ore Mining companies extract iron from iron ore according to the following balanced chemical equation: \[ \text{Fe}_2\text{O}_3(s) + 3\text{CO}(g) \rightarrow 2\text{Fe}(s) + 3\text{CO}_2(g) \] In a reaction mixture containing 169 g of \(\text{Fe}_2\text{O}_3\) and 73.8 g of CO, CO is the limiting reactant. #### Part A Calculate the mass of the reactant in excess (which is \(\text{Fe}_2\text{O}_3\)) that remains after the reaction has gone to completion. Express the mass with the appropriate units.
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