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r-ruslan [8.4K]
3 years ago
10

When 13.0 g of a hydrocarbon are burned in excess O2, 9.0 g of H2O are formed. What is the formula of the hydrocarbon?

Chemistry
1 answer:
givi [52]3 years ago
6 0

Answer:

CH

Explanation:

When a hydrocarbon burns, there are only two products. These are hydrogen and carbon iv oxide. The general equation for burning a hydrocarbon is shown below:

Fuel + O2 → CO2 + H2O

Since 9g Of water is formed, we can get the number of moles of hydrogen and the mass of hydrogen.

We now need to get the actual moles of carbon and hydrogen in the hydrocarbon to know what the chemical formula is.

The number of moles of hydrogen and its mass can be obtained from that of water. The number of moles of water is simply the mass of water divided by the molar mass. The molar mass of water is 18g/mol. The number of moles is thus 9/18 which is 0.5. Since there are two atoms of hydrogen in one molecule of water, the number of moles of hydrogen is thus 2 * 0.5 which equals one mole.

The mass of hydrogen is thus the number of moles of hydrogen * the molar mass of hydrogen which is

1 * 1 = 1g

Hence, the mass of the carbon in the hydrocarbon is 13 - 1 = 12g

The number of moles of carbon present is thus 12/12 which equals 1.

Since the mole ratio is 1 to 1 , the formula of the hydrocarbon is thus CH

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Ammonia and oxygen react to form nitrogen and water.
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Answer:

A. 19.2 g of O2.

B. 3.79 g of N2.

C. 54 g of H2O.

Explanation:

The balanced equation for the reaction is given below:

4NH3(g) + 3O2(g) → 2N2+ 6H2O(g)

Next, we shall determine the masses of NH3 and O2 that reacted and the masses of N2 and H2O produced from the balanced equation.

This is illustrated below:

Molar mass of NH3 = 14 + (3x1) = 17 g/mol

Mass of NH3 from the balanced equation = 4 x 17 = 68 g

Molar mass of O2 = 16x2 = 32 g/mol

Mass of O2 from the balanced equation = 3 x 32 = 96 g

Molar mass of N2 = 2x14 = 28 g/mol

Mass of N2 from the balanced equation = 2 x 28 = 56 g

Molar mass of H2O = (2x1) + 16 = 18 g/mol

Mass of H2O from the balanced equation = 6 x 18 = 108 g

Summary:

From the balanced equation above,

68 g of NH3 reacted with 96 g of O2 to produce 56 g of N2 and 108 g of H2O.

A. Determination of the mass of O2 needed to react with 13.6 g of NH3.

This is illustrated below:

From the balanced equation above,

68 g of NH3 reacted with 96 g of O2.

Therefore, 13.6 g of NH3 will react with = (13.6 x 96)/68 = 19.2 g of O2.

Therefore, 19.2 g of O2 are needed for the reaction.

B. Determination of the mass of N2 produced when 6.50 g of O2 react.

This is illustrated below:

From the balanced equation above,

96 g of O2 reacted to produce 56 g of N2.

Therefore, 6.5 g of O2 will react to produce = (6.5 x 56)/96 = 3.79 g of N2.

Therefore, 3.79 g of N2 were produced from the reaction.

C. Determination of the mass of H2O formed from the reaction of 34 g of NH3.

This is illustrated below:

From the balanced equation above,

68 g of NH3 reacted to 108 g of H2O.

Therefore, 34 g of NH3 will react to produce = (34 x 108)/68 = 54 g of H2O.

Therefore, 54 g of H2O were obtained from the reaction.

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3 years ago
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Answer:

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<u>1) Data:</u>

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<u>2) Formula:</u>

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<u>3) Solution:</u>

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Hence, the mass of the milk is 530.4 g.

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