Question

Silver nitrate reacts with magnesium chloride to form solid silver chloride and aqueous magnesium nitrate. Determine...

Silver nitrate reacts with magnesium chloride to form solid silver chloride and aqueous magnesium nitrate.

Determine the percent yield if a student isolates 58.9 mg of solid silver chloride from the mixture of 0.168 g of silver nitrate and 0.543 g of magnesium chloride.

What mass, in grams, of excess reactant remains?

Homework Answers

Answer #1

The reaction is given as :

2AgNO3 + MgCl2 = 2AgCl + Mg(NO3)2

0.168 g of silver nitrate = 0.168 / 169.87 = 9.89 x 10-4 moles

0.543 g of magnesium chloride = 0.543/ 95.211 = 0.0057 moles or 5.7 x 10-3 moles

1 mole of MgCl2 requires 2 moles of AgNO3 , so 5.7 x 10-3 moles will require 2 x 5.7 x 10-3 = 1.14 x 10-2 moles

So clearly AgNO3 is the limiting reagent.

9.89 x 10-4 moles will make 9.89 x 10-4 moles of AgCl

So the theoretical yield of AgCl = 9.89 x 10-4 x 143.32 = 0.142 g

Percent yield = (0.0589 / 0.142) x 100

= 41.48 %

Number of moles of MgCl2 required = (9.89 x 10-4 ) / 2 = 4.945 x 10-4 moles.

Excess MgCl2 = (5.7 x 10-3) - (4.945 x 10-4)

= 5.2 x 10-3 g

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A 0.271 g piece of solid magnesium reacts with gaseous oxygen from the atmosphere to form...
A 0.271 g piece of solid magnesium reacts with gaseous oxygen from the atmosphere to form solid magnesium oxide. In the laboratory a student weighs the mass of the magnesium oxide collected from this reaction as 0.234 g. What is the percent yield of this reaction?
When solutions of silver nitrate and magnesium chloride are mixed, silver chloride precipitates out of solution...
When solutions of silver nitrate and magnesium chloride are mixed, silver chloride precipitates out of solution according to the equation 2AgNO3(aq)+MgCl2(aq)→2AgCl(s)+Mg(NO3)2(aq). What mass of silver chloride can be produced from 1.96 L of a 0.233 Msolution of silver nitrate? Express your answer with the appropriate units. Mass of AgCl=65.3 The reaction described in Part A required 3.46 L of magnesium chloride. What is the concentration of this magnesium chloride solution? Express your answer with the appropriate units.
When solutions of silver nitrate and magnesium chloride are mixed, silver chloride precipitates out of solution...
When solutions of silver nitrate and magnesium chloride are mixed, silver chloride precipitates out of solution according to the equation 2AgNO3(aq)+MgCl2(aq)→2AgCl(s)+Mg(NO3)2(aq). What mass of silver chloride can be produced from 1.96 L of a 0.233 M solution of silver nitrate? Express your answer with the appropriate units. The reaction described in Part A required 3.46 L of magnesium chloride. What is the concentration of this magnesium chloride solution? Express your answer with the appropriate units.
When solutions of silver nitrate and magnesium chloride are mixed, silver chloride precipitates out of solution...
When solutions of silver nitrate and magnesium chloride are mixed, silver chloride precipitates out of solution according to the equation 2AgNO3(aq)+MgCl2(aq)→2AgCl(s)+Mg(NO3)2(aq) Part A: What mass of silver chloride can be produced from 1.31 L of a 0.156 M solution of silver nitrate? Express your answer with the appropriate units. Part B: The reaction described in Part A required 3.43 L of magnesium chloride. What is the concentration of this magnesium chloride solution? Express your answer with the appropriate units.
What happens to the solid copper and the aqueous silver from the silver nitrate solution during...
What happens to the solid copper and the aqueous silver from the silver nitrate solution during the course of the reaction? A) The copper changed from an aqueous ion form to a solid, metallic state. The metallic silver from the silver nitrate solution became aqueous ions. B) The copper changed from a solid, metallic, unreacted state to and aqeuous ion form. The metallic silver from the silver nitrate solution became aqueous ions. C) The copper changed from a solid, metallic,...
If 32.0 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.211...
If 32.0 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.211 g of precipitate, what is the molarity of silver ion in the original solution?
if 65.1 ml of silver nitrate solution reacts with excess potassium chloride solution to yield 0.365...
if 65.1 ml of silver nitrate solution reacts with excess potassium chloride solution to yield 0.365 g of precipitate,what is the molarity of silver ion in the original solution
If 56.3 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.273...
If 56.3 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.273 g of precipitate, what is the molarity of silver ion in the original solution? ____M
Zinc and magnesium metal each reacts with hydrochloric acid to make chloride salts of the respective...
Zinc and magnesium metal each reacts with hydrochloric acid to make chloride salts of the respective metals, and hydrogen gas. A 10.00-g mixture of zinc and magnesium produces 0.5492 g of hydrogen gas upon being mixed with an excess of hydrochloric acid. Determine the percent magnesium by mass in the original mixture.
Aqueous silver(I) perchlorate reacts with aqueous calcium sulfide to form solid silver(I) sulfide and aqueous calcium...
Aqueous silver(I) perchlorate reacts with aqueous calcium sulfide to form solid silver(I) sulfide and aqueous calcium perchlorate. If 300 mL of 0.200 M silver(I) perchlorate is mixed with 500 mL of 0.300 M calcium sulfide, how many g of silver (I) sulfide will be formed?