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For the reaction shown, calculate how many grams of each

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 35P Chapter 8

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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Problem 35P

PROBLEM 35P

For the reaction shown, calculate how many grams of each product form when the given amount of each reactant completely reacts to form products. Assume there is more than enough of the other reactant.

2 Al(s) + Fe2O3(s) → Al2O3(s) + 2 Fe(l)

(a) 4.7 g Al

(b) 4.7 g Fe2O3

Step-by-Step Solution:

Solution 35P

Here, we are going to calculate the mass of product formed when the given amount of each reactant completely reacts.

Step 1:

a)

The given reaction is:

                        2Al(s) +  Fe2O3(s) → Al2O3(s) + 2Fe(l)

Given, mass of Al = 4.7 g

Molar mass of Al = 26.98 g/mol

Therefore, number of  moles of Al = given mass / molar mass

                                       =  = 0.17 mol

From the above reaction, it is seen that 2 moles of Al produces 1 mole of Al2O3 and 2 moles of Fe.

Therefore, 0.17 mol of Al will produce (½ x 0.17 = 0.085) mol of Al2O3 and 0.17 mol of Fe.

Step 2:

Now, 1 mol Al2O3 = molar mass of Al2O3

Therefore, 0.085 mol of Al2O3 = 0.085 x molar mass of Al2O3

                           = 0.085 x 101.96 g/mol

                           = 8.67 g

Again, 1 mol Fe = molar mass of Fe

Therefore, 0.17 mol of Fe = 0.17 x molar mass of Fe

                              = 0.17 x 55.845 g/mol

                              = 9.49 g

Thus 4.7 g Al produces 8.67 g Al2O3  and 9.49 g Fe.

Step3:

b)

Given, mass of Fe2O3 = 4.7 g

Molar mass of Fe2O3 = 159.69 g/mol

Therefore, number of  moles of Fe2O3 = given mass / molar mass

                                       =  = 0.029 mol

From the above reaction, it is seen that 1 mole of Fe2O3 produces 1 mole of Al2O3 and 2 moles of Fe.

Therefore, 0.029 mol of Fe2O3 will produce 0.029 mol of Al2O3 and (0.029 x 2 = 0.058) mol of Fe.

Step 4:

Now, 1 mol Al2O3 = molar mass of Al2O3

Therefore, 0.029 mol of Al2O3 = 0.029 x molar mass of Al2O3

                           = 0.029 x 101.96 g/mol

                           = 2.96 g

Again, 1 mol Fe = molar mass of Fe

Therefore, 0.058 mol of Fe = 0.058 x molar mass of Fe

                              = 0.058 x 55.845 g/mol

                              = 3.24 g

Thus 4.7 g Fe2O3 produces 2.96 g Al2O3  and 3.24 g Fe.

                         

Step 3 of 4

Chapter 8, Problem 35P is Solved
Step 4 of 4

Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The answer to “For the reaction shown, calculate how many grams of each product form when the given amount of each reactant completely reacts to form products. Assume there is more than enough of the other reactant.2 Al(s) + Fe2O3(s) ? Al2O3(s) + 2 Fe(l)(a) 4.7 g Al(b) 4.7 g Fe2O3” is broken down into a number of easy to follow steps, and 48 words. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. The full step-by-step solution to problem: 35P from chapter: 8 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. Since the solution to 35P from 8 chapter was answered, more than 2002 students have viewed the full step-by-step answer. This full solution covers the following key subjects: form, reactant, grams, completely, enough. This expansive textbook survival guide covers 19 chapters, and 2045 solutions.

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