How many moles of CO2 can be produced by the reaction of 5.00 mol of C2H6 and 12.0 mol of O2 as shown below?C2H6 (g) +5/2 O2-(g)----2CO2 +3H2OGroup of answer choices8310non of the above5

To determine how many moles of CO2 can be produced by the reaction of 5.00 mol of C2H6 and 12.0 mol of O2, we need to follow these steps:

1. Write the balanced chemical equation: $\text{C}_2\text{H}_6 (g) + \frac{5}{2} \text{O}_2 (g) \rightarrow 2 \text{CO}_2 (g) + 3 \text{H}_2\text{O} (g)$

2. Determine the limiting reactant:

   • Calculate the moles of O2 required to react with 5.00 mol of C2H6: $5.00 \text{ mol C}_2\text{H}_6 \times \frac{5}{2} \text{ mol O}_2 \text{ per mol C}_2\text{H}_6 = 12.5 \text{ mol O}_2$
   • Compare the required moles of O2 with the available moles of O2: $\text{Available O}_2 = 12.0 \text{ mol}$
   • Since 12.0 mol of O2 is less than the required 12.5 mol, O2 is the limiting reactant.

3. Calculate the moles of CO2 produced:

   • Use the stoichiometry of the balanced equation to find the moles of CO2 produced from the limiting reactant (O2): $12.0 \text{ mol O}_2 \times \frac{2 \text{ mol CO}_2}{\frac{5}{2} \text{ mol O}_2} = 12.0 \text{ mol O}_2 \times \frac{2}{2.5} = 12.0 \text{ mol O}_2 \times 0.8 = 9.6 \text{ mol CO}_2$

Therefore, the number of moles of CO2 that can be produced is 9.6 mol. However, since this value does not match any of the provided answer choices, it seems there might be an error in the provided choices or the question itself.