# Question ea179

Jul 26, 2016

17%

#### Explanation:

So, you know that the theoretical yield for this reaction is $\text{35.4 g}$. This means that when $\text{20.0 g}$ of lithium hydroxide take part in the reaction, you can expect to produce a maximum of $\text{35.4 g}$ of lithium chloride.

Now, you perform this reaction with this info in mind and find that the reaction produced $\text{6.0 g}$ of lithium chloride. This represents the reaction's actual yield, i.e. what you actually get when you perform the reaction.

The reaction's percent yield essentially tells you how much product you actually get for every $\text{100 g}$ of product that you should theoretically get.

$\textcolor{b l u e}{| \overline{\underline{\textcolor{w h i t e}{\frac{a}{a}} \text{% yield" = "what you actually get"/"what you should theoretically get} \times 100 \textcolor{w h i t e}{\frac{a}{a}} |}}}$

All you have to do now is plug in your values to find

"% yield" = (6 color(red)(cancel(color(black)("g"))))/(35.4color(red)(cancel(color(black)("g")))) xx 100 = color(green)(|bar(ul(color(white)(a/a)color(black)(17%)color(white)(a/a)|)))#

The answer is rounded to two sig figs.

This tells you that for every $\text{100 g}$ of lithium chloride that the reaction could produce, you only get $\text{17 g}$, which constitutes a very, very low percent yield.