# Question #8cb12

##### 1 Answer

#### Explanation:

This is a pretty straightforward **Henry's Law** practice problem in which you have to use the *molar solubility* of the gas and the *partial pressure* of the gas to find the value of **Henry's constant**,

As you know, Henry's Law states that the solubility of a gas in a liquid is **proportional** to that gas' partial pressure above the liquid.

#color(blue)(c = H^(cp) * P)" "# , where

*Henry's constant*

In your case, you have

#H^(cp) = c/P#

Plug in your values to get

#H^(cp) = "0.00140 mol L"^(-1)/("760 mmHg") = "0.000001842 mol L"^(-1)"mmHg"^(-1)#

You need to round this off to two **sig figs**, since that's how many sig figs you have for the partial pressure of the gas.

Expressed in *scientific notation* and rounded to two sig figs, the answer will be

#H^(cp) = color(green)(1.8 * 10^(-6)"mol L"^(-1)"mmHg"^(-1))#