Part 5) How many moles of CO 2 could be produced if 24g of CH 4 were used in the

Question

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?

Explanation / Answer

5)

mass of CH4 = 24 g

molar mass of CH4 = 16 g/mol

mol of CH4 = (mass)/(molar mass)

= 24/16

= 1.5 mol

According to balanced equation

mol of CO2 formed = moles of CH4

= 1.5 mol

Answer: 1.5 mol

6)

mass of CO2 formed = number of mol * molar mass

= 1.5 mol * 44 g/mol

= 66 g

Answer: 66 g

7)

from balanced reaction:

moles of O2 required = moles of H2O formed

moles of O2 required = 2 mol

mass of O2 required = moles of O2 * molar mass of O2

= 2 mol * 32 g/mol

= 64 g

Answer: 64 g

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