Final answer:
The total mass of products formed when 16 grams of CH4 we need to calculate the molar masses of CO2 and H2O. The molar mass of CO2 is 44.01 g/mol and the molar mass of H2O is 18.015 g/mol is burned with excess oxygen in the reaction CH4 + 2O2 = CO2 + 2H2O is 62 grams.
Step-by-step explanation:
The balanced equation for the combustion of CH4 (methane) is: CH4 + 2O2 = CO2 + 2H2O. To find the total mass of products formed, we need to calculate the molar masses of CO2 and H2O. The molar mass of CO2 is 44.01 g/mol and the molar mass of H2O is 18.015 g/mol. For every mole of CH4 burned, we will get one mole of CO2 and two moles of H2O. Therefore, the total mass of products formed will be: Total mass = (1 mol CO2 * 44.01 g/mol) + (2 mol H2O * 18.015 g/mol) = 62 grams, So the correct answer is d) 62 grams.
The total mass of products formed when 16 grams of CH4 we need to calculate the molar masses of CO2 and H2O. The molar mass of CO2 is 44.01 g/mol and the molar mass of H2O is 18.015 g/mol is burned with excess oxygen in the reaction For every mole of CH4 burned, we will get one mole of CO2 and two moles of H2O. Therefore, the total mass of products formed will be: CH4 + 2O2 = CO2 + 2H2O is 62 grams.