A chemist mixes of aluminum metal with of elemental iodine.

1. Write formulas for:

a. elemental aluminum

b. elemental iodine

c. aluminum iodide

2. Write a balanced chemical equation for the reaction

3. How many moles of each reactant were mixed?

a. moles of elemental aluminum:

b. moles of elemental iodine:

4. Demonstrate clearly which reactant is the limiting reagent and the excess reagent.

5. How many grams of product could be formed?(Theoretical yield)

6. How many grams of excess reagent remain?

answer

watching

171

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Jeah BadeoLv10

22 Jan 2021

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

CuCl2.2H2O is reacted with elemental Aluminum to make elemental copper and aqueous aluminum chloride and water.

A student dissolves 0.50 g of CuCl2.2H2O in 20 mL of water. The student adds 3 mL of 3.0 M Hydrochloric Acid. The student then adds in 0.75 g of elemental aluminum. The solution fizzes and the solid aluminum became flaky bits of copper. The copper was rinsed with water and then with acetone to assist in drying the elemental copper. The copper product of the reaction had a mass of 0.15 g

Molar Mass of:
1. CuCl2.2H2O

2. Al
3. AlCl3
4. Cu

Moles of copper added: ____________________________
Moles of Aluminum added: ____________________________
Write the balanced chemical equation for the reaction that is occurring.

Predicted moles of copper that the reaction should have made: ________________________________

Predicted grams of copper that the reaction should have made: ________________________________

Percent Yield of the reaction: __________________________________
Based on the moles of copper the student added to the reaction, how many moles of aluminum SHOULD have been added to the reaction?

Was enough aluminum actually added by the student?

Which reagent limits how much copper the reaction can produce?

14. Show all of your work for each of the following problems. An aluminum nail of mass 5.00g is immersed into a solution of copper(II)nitrate. The mass of copper(II)nitrate in the solution is 6.50g. a. Write the balanced chemical equation for the reaction. b. What is the limiting reactant? c. How many grams of elemental copper can be produced from the reaction? d. How many grams of excess reactant remains when the limiting reactant is consumed? e. What is the % yield if 1.95g of copper is produced from the reaction in the lab?