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mezya [45]
3 years ago
10

A Question Pre

Chemistry
2 answers:
lana66690 [7]3 years ago
7 0

Answer:

A present

Explanation:

Because if the facts

VMariaS [17]3 years ago
5 0

Answer:

Seal them in a glass container in an atmosphere of argon (Ar) gas.

Explanation:

chem

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3. The breaking down of rocks into smaller pieces by physical
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A. Chemical weathering

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3 years ago
An oily liquid with a cheesy, waxy odor like that of goats or other barnyard animals is caproic acid, a compound containing carb
Zinaida [17]

The empirical formula for the caproic acid, given the combustion analysis data is C₃H₆O

We'll begin bey obtaining the mass of carbon, hydrogen and oxygen in the compound. This is illustrated below:

How to determine the mass of C

  • Mass of CO₂ = 9.78 g
  • Molar mass of CO₂ = 44 g/mol
  • Molar of C = 12 g/mol
  • Mass of C =?

Mass of C = (12 / 44) × 9.78

Mass of C = 2.67 g

How to determine the mass of H

  • Mass of H₂O = 20.99 g
  • Molar mass of H₂O = 18 g/mol
  • Molar of H = 2 × 1 = 2 g/mol
  • Mass of H =?

Mass of H = (2 / 18) × 4

Mass of H = 0.44 g

How to determine the mass of O

  • Mass of compound = 4.30 g
  • Mass of C = 2.67 g
  • Mass of H = 0.44 g
  • Mass of O =?

Mass of O = (mass of compound) – (mass of C + mass of H)

Mass of O = 4.30 – (2.67 + 0.44)

Mass of O = 1.19 g

<h3>How to determine the empirical formula </h3>

The empirical formula of the compound can be obtained as follow:

  • C = 2.67 g
  • H = 0.44 g
  • O = 1.19 g
  • Empirical formula =?

Divide by their molar mass

C = 2.67 / 12 = 0.2225

H = 0.44 / 1 = 0.44

O = 1.19 / 16 = 0.074

Divide by the smallest

C = 0.2225 / 0.074 = 3

H = 0.44 / 0.0744 = 6

O = 0.074 / 0.074 = 1

Thus, the empirical formula of the compound is C₃H₆O

Learn more about empirical formula:

brainly.com/question/9459553

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1 year ago
Chemist determined by measurements that 0.015 moles of nickel participated in a chemical reaction. Calculate the mass of nickel
san4es73 [151]

Mass of Ni = 0.015 mol Ni × (58.693 g Ni/1 mol Ni) = 0.88 g Ni

5 0
3 years ago
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