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Combustion of hydrocarbons such as heptane () 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 heptane into gaseous carbon dioxide and gaseous water.


2. Suppose 0.240 kg of heptane are burned in air at a pressure of exactly 1 atm and a temperature of 14.0 °C. Calculate the volume of carbon dioxide gas that is produced. Be sure your answer has the correct number of significant digits.

Respuesta :

Answer:

Explanation:

C₇H₁₆(l) +  11 O₂(g)  =  7CO₂(g) + 8H₂O (g)

100 g                           7 x 22.4 l

At NTP , 100 g of heptane gives 7 x 22.4 liter of carbon dioxide

.24 g of heptane will give        [tex]\frac{7 \times22.4\times.24}{100}[/tex] liter of CO₂

= .376 Litre of carbon dioxide  at NTP .

Given temperature = 287 , pressure 1 atom .  

gas formula

[tex]\frac{P_1V_1}{T_1} = \frac{ P_2V_2} {T_2}[/tex]

[tex]\frac{ 1\times .376}{273} = \frac{ 1\times V_2} {287}[/tex]

V₂ = .395 liter.