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: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter4: Chemical Reactions In Solution
Section: Chapter Questions
Problem 4.21QE
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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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