# Question #d20e1

##### 1 Answer

#### Answer:

**WARNING! Long answer!** The limiting reactant is

#### Explanation:

We know that we will need a balanced equation with masses, moles, and molar masses of the compounds involved.

**1. Gather all the information** in one place with molar masses above the formulas and everything else below them.

We start with the balanced equation.

**(a) Calculate the moles of #"CO"#**

**(b) Calculate moles of #"O"_2#**

**2. Identify the limiting reactant**

An easy way to identify the limiting reactant is to calculate the "moles of reaction" each will give:

You divide the moles of each reactant by its corresponding coefficient in the balanced equation.

I did that for you in the table above.

**3. Calculate the theoretical yield of #"CO"_2#.**

The theoretical yield of

**4. Calculate the percent yield of #"CO"_2#**

The formula for percentage yield is

#color(blue)(bar(ul(|color(white)(a/a)"% yield" = "actual yield"/"theoretical yield" × 100 %color(white)(a/a)|)))" "#

The percent yield is 600 %.

This is an impossible result. Are you sure you gave us the correct data?