Question

Al2(SO4)3+6KOH=2Al(OH)3+3K2SO4 if he added 55.5 g of Aluminum Sulfate to 55.5 g of Potassium hydroxide and...

Al2(SO4)3+6KOH=2Al(OH)3+3K2SO4 if he added 55.5 g of Aluminum Sulfate to 55.5 g of Potassium hydroxide and produced 18.65 g of Aluminum Hydroxide what is the percent yield?

Homework Answers

Answer #1

Al2(SO4)3 + 6 KOH ------------>  2Al(OH)3 + 3K2SO4

first calculate the limiting reagent.

342.15 g Al2(SO4)3 reacts with 6 x 56.1 g KOH

55.5 g Al2(SO4)3 reacts with 55.5 x 6 x 56.1 / 342.15 = 54.6 g KOH

but we have 55.5 g KOH so KOH is exess reagent.

Al2(SO4)3 is limiting reagent.

342.15 g Al2(SO4)3 forms 2 x 78 g Al(OH)3

55.5 g Al2(SO4)3 forms 55.5 x 2 x 78 / 342.15 = 25.5 g

therotical yield = 25.5 g

actual yield = 18.65 g

% yield = (actual yield / therotical yield) x 100

% yield = (18.65 / 25.5) x 100

% yield = 73.14 %

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
Sulfuric acid dissolves aluminum metal according to the following reaction: 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve...
Sulfuric acid dissolves aluminum metal according to the following reaction: 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve an aluminum block with a mass of 15.1 g . What minimum mass of H2SO4 would you need? What mass of H2 gas would be produced by the complete reaction of the aluminum block?
Sulfuric acid dissolves aluminum metal according to the following reaction: 2Al(s)+3H2SO4(aq)--->Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve...
Sulfuric acid dissolves aluminum metal according to the following reaction: 2Al(s)+3H2SO4(aq)--->Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve an aluminum block with a mass of 14.2 g. A) What minimum mass of H2SO4 would you need? B) What mass of H2 gas would be produced by the complete reaction of the aluminum block?
If 1.20 g of aluminum hydroxide reacts with 3.00 g of sulfuric acid, what is the...
If 1.20 g of aluminum hydroxide reacts with 3.00 g of sulfuric acid, what is the mass of water produced? Al(OH)3(s)+H2SO4(l)→Al2(SO4)3(aq)+H2O(l)
Sulfuric acid dissolves aluminum metal according to the following reaction: 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve...
Sulfuric acid dissolves aluminum metal according to the following reaction: 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve an aluminum block with a mass of 14.5 g . Part A What minimum mass of H2SO4 would you need? I got 79.1 g, which is correct. Part B What mass of H2 gas would be produced by the complete reaction of the aluminum block? Express your answer in grams.
Sulfuric acid dissolves aluminum metal according to the following reaction: 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve...
Sulfuric acid dissolves aluminum metal according to the following reaction: 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve an aluminum block with a mass of 15.3 g . Part A: What minimum mass of H2SO4 would you need? Express your answer in grams. Part B: What mass of H2 gas would be produced by the complete reaction of the aluminum block? Express your answer in grams.
A mixture contains only NaCl and Al2(SO4)3. A 1.75-g sample of the mixture is dissolved in...
A mixture contains only NaCl and Al2(SO4)3. A 1.75-g sample of the mixture is dissolved in water, and an excess of NaOH is added, producing a precipitate of Al(OH)3. The precipitate is filtered, dried, and weighed. The mass of the precipitate is 0.134 g. What is the mass percent of Al2(SO4)3 in the sample?
A 500-g sample of aluminum sulfate is reacted with 450 g of calcium hydroxide. If 500...
A 500-g sample of aluminum sulfate is reacted with 450 g of calcium hydroxide. If 500 grams of calcium sulfate are produced, what is the percent yield of the reaction? Please show all work for partial credit.
The experiment calls for preparing one of two salts, either copper(ii) sulfate or potassium aluminum sulfate....
The experiment calls for preparing one of two salts, either copper(ii) sulfate or potassium aluminum sulfate. The instructions for the potassium aluminum sulfate preparation give a target of between 0.025 and 0.050 moles of the product. The instructions also specify to use an excess of potassium hydroxide but not more than 2 times the amount required by the balanced equation. Calculate the mass in grams of aluminum needed to prepare the maximum number of moles of product as noted above....
The experiment calls for preparing one of two salts, either copper(ii) sulfate or potassium aluminum sulfate....
The experiment calls for preparing one of two salts, either copper(ii) sulfate or potassium aluminum sulfate. The instructions for the potassium aluminum sulfate preparation give a target of between 0.025 and 0.050 moles of the product. The instructions also specify to use an excess of potassium hydroxide but not more than 2 times the amount required by the balanced equation. Calculate the mass in grams of aluminum needed to prepare the maximum number of moles of product as noted above....
1.) A student found that the sulfate ion concentration in a solution of Al2(SO4)3 was 0.34...
1.) A student found that the sulfate ion concentration in a solution of Al2(SO4)3 was 0.34 M. What was the concentration of Al2(SO4)3 in the solution? C(Al2(SO4)3)= 2.) To study the effect of dissolved salt on the rusting of an iron sample, a student prepared a solution of NaCl by dissolving 4.250 g of NaCl in enough water to make 204.2 mL of solution. What is the molarity of this solution? C(NaCl) = 3.) A student found that the sulfate...