   # The equation for the reaction of Mg and O 2 , is 2 Mg(s) + O 2 (g) → 2 MgO(s). If you want to prepare 1.0 g of MgO, what mass of magnesium should you use? (a) 030 g Mg (b) 0.20 g Mg (c) 0.40 g Mg (d) 060 g Mg ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 4.1, Problem 2RC
Textbook Problem
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## The equation for the reaction of Mg and O2, is 2 Mg(s) + O2(g) → 2 MgO(s). If you want to prepare 1.0 g of MgO, what mass of magnesium should you use? (a) 030 g Mg (b) 0.20 g Mg (c) 0.40 g Mg (d) 060 g Mg

Interpretation Introduction

Interpretation:

The mass of Mg , required to prepare 1.0gMgO should be determined.

Concept introduction:

• Numberofmole=GivenmassofthesubstanceMolarmass
• The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol).
• For chemical reaction balanced chemical reaction equation written in accordance with the Law of conservation of mass.
• Law of conservation of mass states that for a reaction total mass of the reactant and product must be equal.
• Stoichiometric factor is a relationship between reactant and product which is obtained from the balanced chemical equation for a particular reaction.

### Explanation of Solution

Balanced chemical equation for the given reaction is,

2Mg(s)+O2(g)2MgO(s)

The amount (moles) of MgO produced can be calculated by using the equation

Numberofmole=GivenmassofthesubstanceMolarmass

1.0gMgO×1molMgO40.3044gMgO=0.02481molMgO

Using the stoichiometric factor calculating the amount of magnesium required based on the amount of MgO as follows,

0.02481molMgO×2molMg2molMgO=0

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