Question

the combustion of methane CH₄ releases 890.4 kj/mol. of methane combusted. how much carbon dioxide in grams was produced in a reaction that released 3145 calories?

Answer 1

To determine the mass of carbon dioxide produced, we need to convert the given heat energy to kilojoules, use stoichiometry to calculate the amount of methane burned, and then convert moles of carbon dioxide to grams using the molar mass.

Step-by-step explanation:

When methane gas is combusted, it releases heat energy, making the reaction exothermic. The combustion of 1 mol of methane releases 890.4 kilojoules of heat energy. So, to find out how much carbon dioxide is produced when 3145 calories of heat energy is released, we need to perform stoichiometric calculations.

First, convert the heat energy from calories to kilojoules:

3145 calories × 4.184 J/calorie × 0.001 kJ/J = 13.14 kJ

Now, we can use the given energy change to calculate the amount of methane burned:

13.14 kJ ÷ 890.4 kJ/mol = 0.0147 mol CH4

According to the balanced equation, the molar ratio between methane and carbon dioxide is 1:1. Therefore, the amount of carbon dioxide produced is also 0.0147 mol. Finally, we can convert moles of carbon dioxide to grams using the molar mass:

0.0147 mol × 44.01 g/mol = 0.647 g CO2