A lab student dissolves 0.401 g of AgNO3 in a beaker of water and 0.253 g of MgCl2 in another beaker of water. The student then combines the two solutions, which together form AgCl as a white precipitate. He then isolates the AgCl and finds its mass to be 0.292 g. Here is the equation for the reaction: (First balance the reaction, if needed) AgNO3 (aq) + MgCl2 (aq) →AgCl (s) + Mg(NO3)2 Which starting material is the limiting reagent? What is the theoretical yield of AgCl in this reaction? What was the percent yield of AgCl in this reaction?
A lab student dissolves 0.401 g of AgNO3 in a beaker of water and 0.253 g of MgCl2 in another beaker of water. The student then combines the two solutions, which together form AgCl as a white precipitate. He then isolates the AgCl and finds its mass to be 0.292 g. Here is the equation for the reaction: (First balance the reaction, if needed) AgNO3 (aq) + MgCl2 (aq) →AgCl (s) + Mg(NO3)2 Which starting material is the limiting reagent? What is the theoretical yield of AgCl in this reaction? What was the percent yield of AgCl in this reaction?
General Chemistry - Standalone book (MindTap Course List)
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Chapter4: Chemical Reactions
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Problem 4.141QP: Lead(II) nitrate reacts with cesium sulfate in an aqueous precipitation reaction. What are the...
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A lab student dissolves 0.401 g of AgNO3 in a beaker of water and 0.253 g of MgCl2 in another beaker of water. The student then combines the two solutions, which together form AgCl as a white precipitate. He then isolates the AgCl and finds its mass to be 0.292 g.
Here is the equation for the reaction: (First balance the reaction, if needed)
AgNO3 (aq) + MgCl2 (aq) →AgCl (s) + Mg(NO3)2
- Which starting material is the limiting reagent?
- What is the theoretical yield of AgCl in this reaction?
- What was the percent yield of AgCl in this reaction?
Expert Solution
Step 1) Given
Given that :-
0.401 g of AgNO3
0.253 g of MgCl2
Practical yield of AgCl 0.292 g
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