**Text Transcription for Educational Website:**13. Aluminum metal (Al) reacts with sulfur (S) to produce aluminum sulfide (Al₂S₃) according to this balanced chemical equation:\[ 2 \text{Al} (s) + 3 \text{S} (s) \rightarrow \text{Al}_2\text{S}_3 (s) \]**Question:** How many atoms of aluminum will react completely with 1.33 × 10²³ atoms of sulfur?**Explanation:** This is a stoichiometry problem that involves calculating the amount of aluminum atoms needed to react with a given number of sulfur atoms, based on the balanced chemical equation provided. To find the answer, use the stoichiometric ratio from the equation. For every 3 sulfur atoms, 2 aluminum atoms are required to form aluminum sulfide.

We will solve this question using stoichiometric calculations.

13. Aluminum metal (Al) reacts with sulfur (S) to produce aluminum sulfide (ALS) according to this balanced chemical equation: 2 Al(s) +3 S(s) → AlS(s) How many atoms of aluminum will react completely with 1.33 x 104 atoms of sulfur?

13. Aluminum metal (Al) reacts with sulfur (S) to produce aluminum sulfide (ALS) according to this balanced chemical equation: 2 Al(s) +3 S(s) → AlS(s) How many atoms of aluminum will react completely with 1.33 x 104 atoms of sulfur?

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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