   # Nickel forms a compound with carbon monoxide, Ni x (CO) y . To determine its formula, you carefully heat a 0.0973-g sample in air to convert the nickel to 0.0426 g of NiO and the CO to 0.100 g of CO 2 . What is the empirical formula of Ni x (CO) y ? ### 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, Problem 37PS
Textbook Problem
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## Nickel forms a compound with carbon monoxide, Nix(CO)y. To determine its formula, you carefully heat a 0.0973-g sample in air to convert the nickel to 0.0426 g of NiO and the CO to 0.100 g of CO2. What is the empirical formula of Nix(CO)y?

Interpretation Introduction

Interpretation:

The empirical formula of Nix(CO)y should be determined.

Concept introduction:

• Empirical formula of a compound represents the smallest whole number relative ratio of elements in that compound.
• Amount of substance (in mole) can be calculated by using the following 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).

### Explanation of Solution

Nickel forms a compound with carbon monoxide, having general formula Nix(CO)y

When 0.0973g of given nickel sample is burned in oxygen it will converted to 0.0426g of NiO and carbon monoxide is converted to 0.100gCO2.

From the given masses the amount of NiO andCO2 can be calculated.

Thus, amount of NiO andCO2 isolated from the combustion of given compound are,

0.0426gNiO×1molCO274.6928gCO2=0.00057molNiO0.100gCO2×1molCO244.010gCO2=0.00227molCO2

For every mole of NiO isolated, 1 mol of Ni must have been present in the given compound.

So,

0.00057molNiO×1molNiingivensample1molNiO=0

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