# Question 1a111

Mar 30, 2017

$V = 25.48 L$

#### Explanation:

Because we are at standard temperature and pressure and are given only one set of conditions, we have to use the ideal gas law equation: I should mention that the pressure does not always have units of atm, it depends on the units of pressure given in the gas constant.

List your known and unknown variables.

color(red)("Knowns:"
- Number of moles
- Temperature
- Pressure

color(magenta)("Unknowns:"
Volume of ${H}_{2} O \left(g\right)$

At STP, the temperature is 273K and the pressure is 1 atm.

Because the ideal gas law deals with the number of moles instead of grams, we have to first convert grams of water vapor to moles of water vapor using the molar mass of water, which is 18.01 g/mol

$\text{moles" = 20.484cancel"g"xx"1mol"/(18.01cancel"g}$ = 1.137 mol

Now, rearrange the equation to solve for V:

$\frac{n \times R \times T}{P}$

V = (1.137cancel"mol"xx0.0821Lxxcancel(atm)/cancel(molxxK)xx273cancelK)/(1cancel(atm)#

$V = 25.48 L$