Use the following equation to answer questions : 2 C6H10 + 17 O2 12 CO2 + 10 H2O a) If I do this reaction with 35 grams of C6H10 and 45 grams of oxygen, how many grams of carbon dioxide will be formed? b) What is the limiting reagent? ___________ c) How much of the excess reagent is left over after the reaction is finished? d) If 35 grams of carbon dioxide are actually formed from the reaction, what is the percent yield of this reaction?

Percent yield of the reaction is the percent ratio of actual yield to the theoretical yield.It is calculated to be the experimental yield divided by theoretical yield multiplied by 100%.

The theoretical yield is the amount predicted by a stiochiometric calculation based on the number of moles of all reactants present.

This calculation assumes that only one reaction occurs and that the limiting reactant reacts completely.

The actual yield is the quantity of a product that is obtained from a chemical reaction.

2 C₆H₁₀ + 17 O₂ ⇒ 12 CO₂ + 10 H₂O

1. When you do this calculation for 35 grams of C₆H₁₀, you find that 113 grams of CO2 will be formed.

When you do the calculation for 45 grams of oxygen,You find that 43.7 grams of CO2 will be formed.Because 43.7 grams is the smaller number forming 43.7 grams of product.

2. Oxygen is the limiting reagent

3. 21.4 grams of C₆H₁₀ will be left over.

4. 80.1%

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