Question

5 parts to this one question.

Part 1) For the balanced reaction CH₄(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(g), how many molecules of CH₄ are required to make 2 molecules of H₂O?

Part 2) For the balanced reaction CH₄(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(g), how many moles of CH₄ are required to make 2 moles of H₂O?

Part 3) For the balanced reaction CH₄(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(g) what is the ratio of O₂ to CH₄?

Part 4) Based on that ratio determined in Part 3, how many moles of O₂ are required to completely consume 9 moles of CH₄?

Part 5) If 4 moles of CH₄ were used in the reaction CH₄(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(g), what is the maximum number of moles of CO₂ you could expect the reaction to produce?

Answer 1

Part 1)

CH₄(g) + 2 O₂(g) ----------------> CO₂(g) + 2 H₂O(g),

1 molecule of CH4 is needed to produce 2 molecules of H2O

answer : 1 molecule of CH4

Part 2)

CH₄(g) + 2 O₂(g) --------------> CO₂(g) + 2 H₂O(g),

answer : 1 mol of CH4

Part 3)

CH₄(g) + 2 O₂(g) ------------> CO₂(g) + 2 H₂O(g)

ration of O2 to CH4 = 2 : 1

Part 4)

1 mol CH4 -------------> 2 mol O2

9 mol CH4   ----------->   ??

moles of O2 required = 9 x 2 / 1 = 18 mol

moles of O2 required = 18 mol

Part 5)

1 mol CH4   -------------> 1 mol CO2

4 mol CH4 ----------> 4 mol CO2

moles of CO2 produced = 4 mol