Combustion of hydrocarbons such as methane (CH_4) produces carbon dioxide, a \"g
ID: 1063372 • Letter: C
Question
Combustion of hydrocarbons such as methane (CH_4) 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. Write a balanced chemical equation, including physical state symbols, for the combustion of gaseous methane into gaseous carbon dioxide and gaseous water CH_4 (g) + 2O_2 (g) rightarrow CO_2 (g) + 2H_2O(g) Suppose 0.300 kg of methane are burned in air at a pressure of exactly 1 atm and a temperature of 15.0 degree C Calculate the volume of carbon dioxide gas that is produced. Round your answer to 3 significant digits.Explanation / Answer
1. Balanced chemical equation for combustion of methane
CH4(g) + 2O2(g) --> CO2(g) + 2H2O(g)
2. moles of CH4 combusted = 0.300 kg x 1000/16 g/mol = 18.75 moles
1 mole CH4 gives 1 mole CO2
moles of CO2 generated (n) = 18.75 moles
Pressure (P) = 1 atm
Temperature (T) = 15 oC + 273 = 288 K
R = gas constant
Volume (V) of CO2 generated = ?
Using,
V = nRT/P
= 18.75 x 0.08205 x 288/1 = 443.07 L of CO2 generated