Question

Calculate the mass of oxygen consumed during the above reaction.

CH4 + O2 → CO2 + H2O

A. 64.00 grams
B. 32.00 grams
C. 16.04 grams
D. None of the above

Answer 1

To calculate the mass of oxygen consumed during the given reaction, use the balanced chemical equation and convert moles to grams.

Step-by-step explanation:

To calculate the mass of oxygen consumed during the given reaction:

1. Identify the balanced chemical equation: CH4 + O2 → CO2 + H2O
2. Determine the molar ratio between CH4 and O2 by looking at the coefficients in the balanced equation: 1 mole CH4 reacts with 2 moles O2
3. Convert the given amount of CH4 to moles using its molar mass: Moles of CH4 = 1.00 mol
4. Use the molar ratio to calculate the moles of O2 consumed: Moles of O2 = (1.00 mol CH4) x (2 mol O2 / 1 mol CH4) = 2.00 mol O2
5. Finally, convert the moles of O2 to grams using its molar mass: Mass of O2 = (2.00 mol O2) x (32.00 g O2 / 1 mol O2) = 64.00 grams

Therefore, the mass of oxygen consumed during the reaction is 64.00 grams. The correct answer is A. 64.00 grams.