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Tomtit [17]
2 years ago
13

A sample of strontium bicarbonate weighs 5.0020 mg. How many oxygen atoms are in the sample? I have the answer, but don't unders

tand how to get there.
Chemistry
1 answer:
hodyreva [135]2 years ago
5 0

There are 14.4 * 10^18 oxygen atoms in 5.0020 mg of  strontium bicarbonate.

Mass of strontium bicarbonate Sr(HCO3)2 = 5.0020 mg

Molar mass of strontium bicarbonate Sr(HCO3)2 = 209.6537 g/mol

Number of moles of strontium bicarbonate Sr(HCO3)2 = 5.0020 * 10^-3g/209.6537 g/mol

= 2.3858 * 10^-5 moles

Given that we have 6 oxygen atoms per molecule of Sr(HCO3)2, the total number of oxygen atoms in Sr(HCO3)2 becomes;

2.3858 * 10^-5 moles * 6.02 * 10^23 = 14.4 * 10^18 oxygen atoms

Learn more: brainly.com/question/9743981

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Answer:

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Explanation:

1. Calculate the mass of each element in 2.78 mg of X.

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\text{Moles of C = 1400  mg C}\times\dfrac{\text{1 mmol C}}{\text{12.01 mg C }} = \text{116.6 mmol C}\\\\\text{Moles of H = 234.9 mg H} \times \dfrac{\text{1 mmol H}}{\text{1.008 mg H}} = \text{233.1 mmol H}\\\\\text{Moles of O = 1870 mg O} \times \dfrac{\text{1 mmol O}}{\text{16.00 mg O}} = \text{116 mmol O}

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4. Round the ratios to the nearest integer

C:H:O = 1:2:1

5. Write the empirical formula

The empirical formula is CH₂O.

6. Calculate the molecular formula.

EF Mass = (12.01 + 2.016  + 16.00) u  = 30.03 u

The molecular formula is an integral multiple of the empirical formula.

MF = (EF)ₙ

n = \dfrac{\text{MF Mass}}{\text{EF Mass }} = \dfrac{\text{150 u}}{\text{30.03 u}} = 5.00  \approx 5

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