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Magnesium oxide can be produced by heating magnesium metal

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

Solution for problem 66P 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 66P

PROBLEM 66P

Magnesium oxide can be produced by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is:

2 Mg(s) + O2(g) → 2 MgO(s)

When 10.1 g of Mg react with 10.5 g of O2, 11.9 g of MgO are collected. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

Step-by-Step Solution:

Solution 66P

Step 1:

In this question the given mass of Mg = 10.1g

                        The mass of O2 = 10.5 g

                         Mass of MgO = 11.9 g

This is very simple, first do the theoretical yield since you need this number to get the percent yield.

We have to determine moles of reactants to see which (if any) is a limiting reagent. They stated it reacted with a certain amount of O2, they didn't say burned in air so you can't assume oxygen is present in excess!

The atomic weight of Mg = 24.305 g/mol and for O2 = 32.0g/mol

Hence number of mol of Mg = 10.1g/24.3g/mole =0.415 mole Mg

Similarly number of mole of O2 = 10.5g/32.0g/mole = 0.328 mole O2

From the balanced equation, you can see that 2 Mg's react with each O2 so 0.328 mole of O2 is more than enough to convert all the Mg to MgO; Mg is the limiting reagent.

Step 2:

Since the ratio of Mg reacted to MgO formed is 1 to 1 we would get 0.415 mole of MgO from 0.415 mole of Mg.

0.415mole  [24.3 + 16.0]g/mole = 16.72g

So the theoretical yield (most MgO you could recover if reaction was 100% complete and no losses in recovering etc) is 16.72g

Step 3 of 3

Chapter 8, Problem 66P is Solved
Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

Since the solution to 66P from 8 chapter was answered, more than 358 students have viewed the full step-by-step answer. The answer to “Magnesium oxide can be produced by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is:2 Mg(s) + O2(g) ? 2 MgO(s)When 10.1 g of Mg react with 10.5 g of O2, 11.9 g of MgO are collected. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.” is broken down into a number of easy to follow steps, and 55 words. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. This full solution covers the following key subjects: Yield, reaction, mgo, magnesium, oxide. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The full step-by-step solution to problem: 66P from chapter: 8 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM.

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