Question

Problem: Given the following chemical reaction between aluminum sulfide and water, if we are given 65.80 g of Al2S3: a) How many moles of water are required for the reaction? b) What mass of H2S & Al(OH)3 would be formed? Al2S3(s) + 6 H2O(l) -> 2 Al(OH)3(s) + 3 H2S(g)

Name: Problem: Given the following chemical reaction between aluminum sulfide and water, if we are given 65.80 g of Al2S3: a) How many moles of water are required for the reaction? b) What mass of H2S Al(OH)3 would be formed? Al2S3(s) + 6 H2O(l) -> 2 Al(OH)3(s) + 3 H2S(g)
Uploaded: 2022-12-30T22:52:28-08:00
Duration: 4 min 15 s
Channel: David Collins
Description: Problem: Given the following chemical reaction between aluminum sulfide and water, if we are given 65.80 g of Al2S3: a) How many moles of water are required for the reaction? b) What mass of H2S Al(OH)3 would be formed? Al2S3(s) + 6 H2O(l) -> 2 Al(OH)3(s) + 3 H2S(g)

          Problem: Given the following chemical reaction between aluminum sulfide and water, if we are given 65.80 g of Al2S3: a) How many moles of water are required for the reaction? b) What mass of H2S & Al(OH)3 would be formed? Al2S3(s) + 6 H2O(l) -> 2 Al(OH)3(s) + 3 H2S(g)

Problem: Given the following chemical reaction between aluminum sulfide and water, if we are given 65.80 g of Al2S3: a) How many moles of water are required for the reaction? b) What mass of H2S Al(OH)3 would be formed? Al2S3(s) + 6 H2O(l) -> 2 Al(OH)3(s) + 3 H2S(g)

Added by Diana C.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

12/30/2022

Step 1

Aluminum sulfide has a mass of 65.80 g and water has a mass of 1 g. Therefore, the moles of water required for the reaction is 6.58 g. Show more…

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Problem: Given the following chemical reaction between aluminum sulfide and water; if we are given 65.80 g of Al2S3: a) How many moles of water are required for the reaction? b) What mass of H2S & Al(OH)3 would be formed? Al2S3 (s) + 6 H2O (l) -> 2 Al(OH)3 (s) + 3 H2S (g)