Final answer:
When 32 grams of methane is burnt, 88 grams of carbon dioxide (CO2) are released according to the stoichiometry of the balanced chemical reaction.
Step-by-step explanation:
To determine how much CO2 is released when 32 grams of methane is burnt, we can use the stoichiometry of the balanced chemical reaction for the combustion of methane. The balanced equation for this exothermic reaction is:
CH4 + 2O2 → CO2 + 2H2O
According to the equation, one mole of methane (CH4) combusts to form one mole of carbon dioxide (CO2). The molar masses are 16 g/mol for methane and 44 g/mol for CO2. Using the stoichiometry of the reaction, we find that 32 grams of methane (which is equivalent to 2 moles, since 32 g ÷ 16 g/mol = 2 mol) will produce 2 moles of CO2. Since the molar mass of CO2 is 44 g/mol, the amount of CO2 produced from 2 moles is:
2 mol × 44 g/mol = 88 grams of CO2
Therefore, burning 32 grams of methane will release 88 grams of carbon dioxide.