Question

10 parts to this one question

Part 1) What is the maximum number of moles of H₂O you could expect the reaction to produce if 4 moles of CH₄ were used?

Part 2 ) If only 0.5 moles of O₂ 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?

Part 3) What is the maximum number of moles of H₂O you could expect the reaction to produce if 0.5 moles of O₂ were used?

Part 4) How many moles are contained in 24 g CH₄?

Part 5) How many moles of CO₂ could be produced if 24g of CH₄ were used in the reaction CH₄(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(g)?

Part 6) How many of grams of CO₂ are contained in the number of moles you calculated in Q11?

Part 7) How many grams of O₂ would have to be used in the reaction CH₄(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(g) to produce 2 moles of H₂O?

Part 8) For the balanced reaction 4 Fe(s) + 3 O₂(g) → 2 Fe₂O₃(s), how many grams of Fe₂O₃ can be produced from 100 g Fe?

Part 9) How many grams of O₂ are required to react with 100 g Fe in this reaction?

Part 10)

Conceptual Model - Xtreme Elmo

If a factory making Xtreme Elmos has 10,000 bodies and 9000 circuit boards, only a limited number of complete products can be made If a clinic has 100 flu shots and 300 patients wanting them, someone will be doing without. In both cases it is obvious what is limiting. In chemical reactions, the only additional step to understanding which is limiting is converting the mass of a substance to the number of moles of that substance. Only moles can be compared, not masses.

What number of Xtreme Elmos could the factory above produce? What limited output?

Answer 1

Part 1) What is the maximum number of moles of H2O you could expect the reaction to produce if 4 moles of CH4 were used?

CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)

from this reaction, we can assume that for 1 mol of CH4 produced, we can proeuce 2 mol of H2O

so

4 mol of CH4 --> 4x2 = 8 mol of H2O can be produced at 100% conversion

Part 2 ) If only 0.5 moles of O2 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?

2 mol of O2 will form 1 mol of CO2

that is, 2:1 ratio

0.5 mol of O2 --> 1/2*0.5 = 0.25 mol of CO2 will be produced

Part 3) What is the maximum number of moles of H2O you could expect the reaction to produce if 0.5 moles of O2 were used?

CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)

2 mol of O2 produced 2 mol of H2O

so; 0.5 mol of O2 will produced 0.5 mol of H2O

Part 4) How many moles are contained in 24 g CH4?

1 mol of CH4 = 16 g

x mol = 24 g

x = 24/16 = 1.5 moles of CH4