Final answer:
The total mass of products formed when 16 grams of CH4 is burned with excess oxygen is 80 grams. Therefore, the total mass of products formed is 44.01 g + 36.04 g = 80.05 g. Rounding to the nearest gram gives us a total mass of 80 grams.
Step-by-step explanation:
To find the total mass of products formed when 16 grams of CH4 is burned with excess oxygen, we need to balance the chemical equation and calculate the number of moles of CH4. The balanced equation for the combustion of CH4 is:
CH4 + 2O2 -> CO2 + 2H2O
From the equation, we can see that 1 mole of CH4 produces 1 mole of CO2 and 2 moles of H2O. Using the molar masses of C, H, and O, we can calculate the mass of CO2 and H2O produced:
1 mole of CO2 = 1 * (12.01 + 2 * 16.00) g = 44.01
2 moles of H2O = 2 * (2 * 1.01 + 16.00) g = 36.04 g
Therefore, the total mass of products formed is 44.01 g + 36.04 g = 80.05 g. Rounding to the nearest gram gives us a total mass of 80 grams.