5 parts to this one question. Part 1) For the balanced reaction CH 4 (g) + 2 O 2

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?

Explanation / Answer

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

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