Aluminum hydroxide reacts with sulfuric acid as follows:

Questions:
A) Which reagent is the limiting reactant when 0.500 mol Al(OH)₃ and 0.500 mol H₂SO₄ are allowed to react?
B) How many moles of Al₂(SO₄)₃ can form under these conditions?
C) How many moles of the excess reactant remain after the completion of the reaction
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Question

Aluminum hydroxide reacts with sulfuric acid as follows:

Questions:
A) Which reagent is the limiting reactant when 0.500 mol Al(OH)₃ and 0.500 mol H₂SO₄ are allowed to react?
B) How many moles of Al₂(SO₄)₃ can form under these conditions?
C) How many moles of the excess reactant remain after the completion of the reaction

chocolatescorpion616

Aluminum hydroxide reacts with sulfuric acid as follows: 2Al(OH)3(s)+3H2SO4(aq)âAl2(SO4)3(aq)+6H2O(l) How many moles of Al2(SO4)3 can form under these conditions? How many moles of the excess reactant remain after the completion of the reaction?

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Aluminum hydroxide reacts with sulfuric acid as follows: 2Al(OH)3(s)+3H2SO4(aq)âAl2(SO4)3(aq)+6H2O(l) How many moles of Al2(SO4)3 can form under these conditions? How many moles of the excess reactant remain after the completion of the reaction?

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

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Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

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Related questions

Weekly leaderboard

Aluminum hydroxide reacts with sulfuric acid as follows: 2Al(OH)3(s)+3H2SO4(aq)âAl2(SO4)3(aq)+6H2O(l) How many moles of Al2(SO4)3 can form under these conditions? How many moles of the excess reactant remain after the completion of the reaction?