Problem: Sulfuric acid cannot be stored in an aluminum container because sulfuric acid dissolves aluminum metal. The following equation shows the reaction: 2 Al (s) + 3 H2SO4 (aq) → Al2(SO4)3 (aq) + 3 H2 (g) Calculate the volume of sulfuric acid that would be required to completely dissolve a 4.643 g block of aluminum if you are given a 0.98 M H2SO4 solution. A. 175.60 mL B. 710.66 mL C. 284.48 mL D. 263.40 mL E. 242.33 mL

🤓 Based on our data, we think this question is relevant for Professor Zimmerman's class at HAWAII.

Problem Details

Sulfuric acid cannot be stored in an aluminum container because sulfuric acid dissolves aluminum metal. The following equation shows the reaction:

2 Al (s) + 3 H2SO4 (aq) → Al2(SO4)3 (aq) + 3 H2 (g)

Calculate the volume of sulfuric acid that would be required to completely dissolve a 4.643 g block of aluminum if you are given a 0.98 M H2SO4 solution.

A. 175.60 mL
B. 710.66 mL
C. 284.48 mL
D. 263.40 mL
E. 242.33 mL

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Solution Stoichiometry concept. You can view video lessons to learn Solution Stoichiometry. Or if you need more Solution Stoichiometry practice, you can also practice Solution Stoichiometry practice problems.

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What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Zimmerman's class at HAWAII.