What mass of precipitate (in g) is formed when 55.8 mL of 0.500 M AIBr, reacts with excess AgNO, in the following chemical reaction? AlBr (aq) + 3 AgNO,(aq) — 3 AgBr(s) + Al(NO,),(aq)
What mass of precipitate (in g) is formed when 55.8 mL of 0.500 M AIBr, reacts with excess AgNO, in the following chemical reaction? AlBr (aq) + 3 AgNO,(aq) — 3 AgBr(s) + Al(NO,),(aq)
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter3: Chemical Reactions
Section: Chapter Questions
Problem 57QRT
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Transcribed Image Text:**Chemical Reaction Problem**
**Question:**
What mass of precipitate (in g) is formed when 55.8 mL of 0.500 M AlBr₃ reacts with excess AgNO₃ in the following chemical reaction?
**Chemical Reaction:**
AlBr₃(aq) + 3 AgNO₃(aq) → 3 AgBr(s) + Al(NO₃)₃(aq)
**Explanation:**
This problem involves a chemical reaction where aluminum bromide (AlBr₃) reacts with silver nitrate (AgNO₃) to form silver bromide (AgBr) as a precipitate and aluminum nitrate (Al(NO₃)₃) in aqueous form. The goal is to calculate the mass of the silver bromide precipitate produced from the given quantities.
To solve this problem:
1. Calculate the moles of AlBr₃ using its concentration and volume.
2. Use stoichiometry from the balanced chemical equation to find the moles of AgBr produced.
3. Convert the moles of AgBr to grams using its molar mass.
This process will determine the amount of precipitate formed in the reaction.
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