   Chapter 4, Problem 94GQ ### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# In an experiment, 1.056 g of a metal carbonate, containing an unknown metal M, is heated to give the metal oxide and 0.376 g CO2.MCO3(s) + heat → MO(s) + CO2(g)What is the identity of the metal M?(a) M = Ni(b) M = Cu(c) M = Zn(d) M = Ba

Interpretation Introduction

Interpretation:

The metal in the given reaction has to be identified.

Concept introduction:

• The number of moles of any substance can be determined using the equation.

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).
• Molarmass=GivenmassofthesubstanceMoleofthesubstance
• 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.

Barium (option d) is the metal involved in the given reaction.

Explanation

Reason for the correct option:

Amount of CO2 available = 0.37644.01 = 0.00854 mol of CO2

Balanced chemical equation for the given reaction is,

MCO3(s)+heatMO(s)+CO2(g)

From the balanced equation it is clear that metal and carbon dioxide are reacting in the ratio of 1:1

The amount of metal can be calculated from the amount of CO2

Therefore,

The amount of  Metal = 0.00854molofCO2×1molMetal1molCO2 = 0.00854molMetal

It is possible to identify an element or compound by its molar mass

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