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Sulfuric acid can dissolve aluminum metal according to the reaction:2 Al(s) + 3
Chapter 8, Problem 41P(choose chapter or problem)
Sulfuric acid can dissolve aluminum metal according to the reaction:
\(2 \mathrm{Al}(\mathrm{s})+3 \mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+3 \mathrm{H}_{2}(g)\)
Suppose you wanted to dissolve an aluminum block with a mass of 22.5 g. What minimum amount of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) in grams do you need? How many grams of \(\mathrm{H}_{2}\) gas will be produced by the complete reaction of the aluminum block?
Questions & Answers
QUESTION:
Sulfuric acid can dissolve aluminum metal according to the reaction:
\(2 \mathrm{Al}(\mathrm{s})+3 \mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+3 \mathrm{H}_{2}(g)\)
Suppose you wanted to dissolve an aluminum block with a mass of 22.5 g. What minimum amount of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) in grams do you need? How many grams of \(\mathrm{H}_{2}\) gas will be produced by the complete reaction of the aluminum block?
ANSWER:
Step 1 of 3
The equation for the reaction between sulfuric acid and aluminum is
Mass of the aluminum block needed to be dissolved by sulfuric acid is .