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9966 [12]
2 years ago
13

A sample of a compound is analyzed and found to contain 0.420 g nitrogen, 0.480g oxygen, 0.540 g carbon and 0.135 g hydrogen. Wh

at is the empirical formula of the compound? a. C2H5NO b. CH3NO c. C3H9N2O2 d. C4HN3O4 e. C4H13N3O3
Chemistry
1 answer:
Crazy boy [7]2 years ago
7 0

Answer:

c. C3H9N2O2

Explanation:

The empirical formula of a compound is defined as the simplest whole number ratio of atoms present in a molecule. To solve this question we need to convert the mass of each atom to moles. With the moles we can find the ratio as follows:

<em>Moles N -Molar mass: 14.01g/mol-</em>

0.420g N * (1mol/14.01g) = 0.0300 moles N

<em>Moles O -Molar mass: 16g/mol-</em>

0.480g O * (1mol/16g) = 0.0300 moles O

<em>Moles C -Molar mass: 12.01g/mol-</em>

0.540g C * (1mol/12.01g) = 0.0450 moles C

<em>Moles H -Molar mass: 1.0g/mol-</em>

0.135g H * (1mol/1g) = 0.135moles H

Dividing in the moles of N (Lower number of moles) the ratio of atoms is:

N = 0.0300 moles N / 0.0300 moles N = 1

O = 0.0300 moles O / 0.0300 moles N = 1

C = 0.0450 moles C / 0.0300 moles N = 1.5

H = 0.135 moles H / 0.0300 moles N = 4.5

As the empirical formula requires whole numbers, multiplying each ratio twice:

N = 2, O = 2, C = 3 and H = 9

And the empirical formula is:

<h3>c. C3H9N2O2</h3>

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2Al + 6HCl --&gt; 2AlCl3 + 3H2 Aluminium reacts with hydrochloric acid. How many grams of aluminum are necessary to produce 11 L
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Answer:

8.8g of Al are necessaries

Explanation:

Based on the reaction, 2 moles of Al are required to produce 3 moles of hydrogen gas.

To solve this question we must find the moles of H2 in 11L at STP using PV = nRT. With these moles we can find the moles of Al required and its mass as follows:

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<em />

<em>Moles Al:</em>

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<em />

<em>Mass Al -Molar mass: 26.98g/mol-:</em>

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