Combustion of hydrocarbons such as nonane (CoH20) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap the Sun's heat, raising the average temperature of the Earth. For this reason, there has been a great deal of international discussion about whether to regulate the production of carbon dioxide. 1. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid nonane into gaseous carbon dioxide and gaseous water. Suppose 0.130 kg of nonane are burned in the air at a pressure of exactly 1 atm and a temperature of 12.0 °C. Calculate the volume of carbon dioxide gas that is produced Be sure your answer has the correct number of significant digits.

1. C9H20 (l) + 14O2 (g) - > 9CO2 (g) + 10H2O (g)

2. 213.70L of CO2

Explanation:

1. The equation for the combustion of liquid nonane into gaseous carbon dioxide and gaseous water is given below:

C9H20 (l) + O2 (g) - > CO2 (g) + H2O (g)

The equation can be balanced as follow:

There are 9 atoms of C on the left side and 1 atom on the right side. It can be balance by putting 9 in front of CO2 as shown below:

C9H20 (l) + O2 (g) - > 9CO2 (g) + H2O (g)

There are 20 atoms of H on the left side and 2 atoms on the right side. It can be balance by putting 10 in front of H2O as shown below:

C9H20 (l) + O2 (g) - > 9CO2 (g) + 10H2O (g)

Now, there are a total of 28 atoms of O on the right side and 2 atoms on the left side. It can be balance by putting 14 in front of O2 as shown below:

C9H20 (l) + 14O2 (g) - > 9CO2 (g) + 10H2O (g)

Now the equation is balanced.

2. Let us convert 0.130 kg of nonane (C9H20) to mole. This is illustrated below:

Molar Mass of C9H20 = (12x9) + (20x1) = 108 + 20 = 128g/mol

Mass of C9H20 from the question =

0.130kg = 0.130 x 1000 = 130g

Mole of C9H20 = ?

Number of mole = Mass/Molar Mass

Mole of C9H20 = 130/128 = 1.016 mole

The equation for the reaction is:

C9H20 (l) + 14O2 (g) - > 9CO2 (g) + 10H2O (g)

From the balanced equation above,

1 mole of C9H20 produced 9 moles of CO2.

Therefore, 1.016 mole of C9H20 will produce = 1.016 x 9 = 9.144 moles

Now, let us calculate the volume of CO2 formed. This is illustrated below:

Data obtained from the question include:

P (pressure) = 1atm

T (temperature) = 12°C = 285K

n (number of mole of CO2) = 9.144 moles

R (gas constant) = 0.082atm. L/Kmol

V (volume of CO2) = ?

Using the ideal gas equation PV = nRT, the volume of CO2 can be obtained as follow:

PV = nRT

1 x V = 9.144 x 0.082 x 285

V = 213.70L

Therefore, 213.70L of CO2 is produced