For each reaction, calculate the moles of product (in parentheses) when 2.00 moles of each reactant is used

A: 2SO2 + O2 = 2SO3 (SO3)
B: 3Fe + 4H2O = Fe3O4 + 4H2 (Fe3O4)
C: C7H16 + 11O2 = 7CO2 + 8H2O (CO2)

Didn't Bob Pursley do one like this for you. You should have learned how to do it from that. Explain what your trouble is.

This is a limiting reagent problem. Here is a site that explain exactly how do do those.

http://www.jiskha.com/science/chemistry/limiting_reagent_problem.html

To calculate the moles of product for each reaction when 2.00 moles of each reactant is used, we need to use the coefficients of the balanced chemical equations.

A: 2SO2 + O2 → 2SO3
In this equation, the coefficient of SO3 in the balanced equation is 2. So, for every 2 moles of SO2 reacted, 2 moles of SO3 will be produced. Since we are using 2.00 moles of SO2, we expect to produce 2.00 moles of SO3.

B: 3Fe + 4H2O → Fe3O4 + 4H2
In this equation, the coefficient of Fe3O4 in the balanced equation is 1. So, for every 3 moles of Fe reacted, 1 mole of Fe3O4 will be produced. Since we are using 2.00 moles of Fe, we need to find the moles of Fe3O4 using a ratio.

Ratio:
3 moles of Fe → 1 mole of Fe3O4
2.00 moles of Fe → x moles of Fe3O4

Using the ratio, we can solve for x:
x = (2.00 moles of Fe) × (1 mole of Fe3O4 / 3 moles of Fe)
x ≈ 0.67 moles of Fe3O4

Therefore, when 2.00 moles of Fe reacts, we expect to produce approximately 0.67 moles of Fe3O4.

C: C7H16 + 11O2 → 7CO2 + 8H2O
In this equation, the coefficient of CO2 in the balanced equation is 7. So, for every 1 mole of C7H16 reacted, 7 moles of CO2 will be produced. Since we are using 2.00 moles of C7H16, we need to find the moles of CO2 using a ratio.

Ratio:
1 mole of C7H16 → 7 moles of CO2
2.00 moles of C7H16 → x moles of CO2

Using the ratio, we can solve for x:
x = (2.00 moles of C7H16) × (7 moles of CO2 / 1 mole of C7H16)
x = 14.00 moles of CO2

Therefore, when 2.00 moles of C7H16 reacts, we expect to produce 14.00 moles of CO2.