Question

2 Al + 3 CuCl2.H2O → 3 Cu + 2 AlCl3 + 6 H2O Assuming 58.99...

2 Al + 3 CuCl2.H2O → 3 Cu + 2 AlCl3 + 6 H2O

Assuming 58.99 grams of Al are consumed in the presence of excess copper II chloride dihydrate, how many grams of AlCl3 can be produced if the reaction will only produce 13.74 % yield?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
You react 150 grams of chlorine with aluminum, 2 Al(s) + 3 Cl2(g)  2 AlCl3(s),...
You react 150 grams of chlorine with aluminum, 2 Al(s) + 3 Cl2(g)  2 AlCl3(s), and get 75 grams of product. What is the actual yield for this reaction? a. 50% b. 75 grams c. 150 grams d. 189 grams
Preparation of Copper(I) Chloride Reactions: 1) Cu(S) + 4HNO3(aq) -> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) 2)...
Preparation of Copper(I) Chloride Reactions: 1) Cu(S) + 4HNO3(aq) -> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) 2) 2HNO3(aq) + Na2CO3(s) -> H2O(l) + CO2(g) + 2NaNO3(aq) 3)Cu(NO3)2(aq) + Na2CO3(s) -> CuCO3(s) + 2NANO3(aq) 4)CuCO3(s) + 2HCL(aq) -> CuCl2(aq) + H2O(l) + CO2(g) 5)CuCl2(aq) + Cu(s) -> 2CuCl(s) Report: Weight of Copper: 1.067g Volume of Added Nitric Acid: 5.0mL Total weight of added Sodium Carbonate: 3.929g Weight of watch glass and filter paper: 51.204g Weight of watch glass, filter paper, and CuCl...
iii) Calculate ΔH for the reaction 2 Al (s) + 3 Cl2 (g) → 2 AlCl3...
iii) Calculate ΔH for the reaction 2 Al (s) + 3 Cl2 (g) → 2 AlCl3 (s) from the data 2 Al (s) + 6 HCl (aq) → 2 AlCl3 (aq) + 3 H2 (g) ΔH = -1049. kJ HCl (g) → HCl (aq) ΔH = -74.8 kJ H2 (g) + Cl2 (g) → 2 HCl (g) ΔH = -1845. kJ AlCl3 (s) → AlCl3 (aq) ΔH = -323. kJ
2 Al(s) + 6 HCl(aq) --> 2 AlCl3(aq) + 3 H2(g) Fe(s) + 2 HCl(aq) -->...
2 Al(s) + 6 HCl(aq) --> 2 AlCl3(aq) + 3 H2(g) Fe(s) + 2 HCl(aq) --> FeCl2(aq) + H2(g) When a 7.007-g sample of a particular iron-aluminum alloy was dissolved in excess hydrochloric acid, 0.4705 g of H2(g) was produced. What was the mass percentage of aluminum in the alloy?
Consider the following reaction: 3Cu(NO3)2 (aq) + 2CrCI3 (aq) ---> 3CuCI2 (s) + 2Cr(NO3)3 (aq) -In...
Consider the following reaction: 3Cu(NO3)2 (aq) + 2CrCI3 (aq) ---> 3CuCI2 (s) + 2Cr(NO3)3 (aq) -In the lab you mixed 36 grams of copper (II) nitrate with an excess amount of chromium(III) chloride. How many moles of chromium(III) nitrate would you produce. -What is the percent yield if you actually produced 15.5 g of chromium(III) nitrate?
1) Cu(S) + 4HNO3(aq) -> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) 2) 2HNO3(aq) + Na2CO3(s) -> H2O(l)...
1) Cu(S) + 4HNO3(aq) -> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) 2) 2HNO3(aq) + Na2CO3(s) -> H2O(l) + CO2(g) + 2NaNO3(aq) 3)Cu(NO3)2(aq) + Na2CO3(s) -> CuCO3(s) + 2NANO3(aq) 4)CuCO3(s) + 2HCL(aq) -> CuCl2(aq) + H2O(l) + CO2(g) 5)CuCl2(aq) + Cu(s) -> 2CuCl(s) weight of copper 1.022g volume of added nitric acid   5.3 ml total weight of added sodium carbonate 4.873g weight of watch glass and filter paper 25.372g Weight of watch glass, filter paper, and CuCl precipitate 53.650 g What is...
Nitric acid reacts violently with copper metal to produce copper (II) nitrate and a noxious brown...
Nitric acid reacts violently with copper metal to produce copper (II) nitrate and a noxious brown gas, NO2. If 8.421 g of copper react with excess nitric acid and the percent yield of NO2 is 71.55% how many grams of NO2 were formed? 4 HNO3+Cu --> Cu(NO3)2+ 2 NO2+ 2 H2O
Given the following experimentally determined values, answer the questions. .009070 mol Cl .00565 mol Cu .00385...
Given the following experimentally determined values, answer the questions. .009070 mol Cl .00565 mol Cu .00385 mol Zn Ratio of Chloride to copper = 1.61:1 Ratio of chloride to zinc = 2.36:1 Ratio of zinc to copper = .681:1 What are your experimentally-determined formulas for (i) copper chloride, and (ii) zinc chloride? Once you have calculated the moles of each element/ion (Cu, Zn, and Cl– ), you can then determine the empirical formula of copper chloride by computing the ratio...
Reaction 1. a) For each mole of Cu dissolved in the nitric acid solution (HNO3), how...
Reaction 1. a) For each mole of Cu dissolved in the nitric acid solution (HNO3), how many moles of [Cu(H2O)6]2+ are formed? b) Given your data above, how many moles of [Cu(H2O)6]2+ were formed in your reaction? Reaction I: Cu (s) + 4 H3O+(aq) + 2 NO3-(aq) --> [Cu(H2O)6]2+(aq) + 2 NO2(g) The first reaction in the series is an oxidation – reduction reaction where copper metal“dissolves” in nitric acid (HNO3). Anoxidation – reduction reactionoccurs when one atomgains an electron...
Assuming a yield of 32.1% 32.1% , calculate the actual yield of magnesium nitrate in grams...
Assuming a yield of 32.1% 32.1% , calculate the actual yield of magnesium nitrate in grams formed from 148.5 g 148.5 g of magnesium and excess copper(II) nitrate. Mg+Cu ( NO 3 ) 2 ⟶Mg ( NO 3 ) 2 +Cu actual yield of Mg(NO3)2Mg(NO3)2 : ____g
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT