# What is the volume at STP of 2.66 mol of methane gas?

Jul 29, 2016

$V = 59.6 L$

#### 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(purple)("Knowns:"
- Number of moles
- Temperature
- Pressure

color(blue)("Unknowns:"
Volume of $C {H}_{4} \left(g\right)$

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

Let's rearrange the equation to solve for V:

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

V = (2.66cancel"mol"xx0.0821Lxxcancel(atm)/cancel(molxxK)xx273cancelK)/(1cancel(atm)

$V = 59.6 L$

Aug 6, 2016

Because the temperature and pressure are given as STP, all that is need is to use the molar volume.

#### Explanation:

1 mole = 22.4 liters.

so  2.66 moles / 1.00 mole =

$$ V/ 22.4#


2.66 x 22.4 = 59.58 liters.