Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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**Question:** What volume (in mL) of 0.200 M HCl would be required to completely react with 6.65 g of Al in the following chemical reaction? \[ 2 \text{Al(s)} + 6 \text{HCl(aq)} \rightarrow 2 \text{AlCl}_3 \text{(aq)} + 3 \text{H}_2 \text{(g)} \] **Explanation:** The question presents a stoichiometry problem involving the reaction of aluminum (Al) with hydrochloric acid (HCl) to form aluminum chloride (AlCl₃) and hydrogen gas (H₂). Given the mass of aluminum, the task is to find the volume of 0.200 M HCl needed for the reaction. This involves calculating moles of aluminum and using the balanced equation to determine moles of HCl required, followed by using the molarity to convert to volume in mL.
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Transcribed Image Text:**Question:** What volume (in mL) of 0.200 M HCl would be required to completely react with 6.65 g of Al in the following chemical reaction? \[ 2 \text{Al(s)} + 6 \text{HCl(aq)} \rightarrow 2 \text{AlCl}_3 \text{(aq)} + 3 \text{H}_2 \text{(g)} \] **Explanation:** The question presents a stoichiometry problem involving the reaction of aluminum (Al) with hydrochloric acid (HCl) to form aluminum chloride (AlCl₃) and hydrogen gas (H₂). Given the mass of aluminum, the task is to find the volume of 0.200 M HCl needed for the reaction. This involves calculating moles of aluminum and using the balanced equation to determine moles of HCl required, followed by using the molarity to convert to volume in mL.
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Molarity of HCl = 0.200 mol/L

Mass of Al = 6.65 g

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