Question

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

Answer 1

`V= 59.6L`

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 `CH_4(g)`

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

Let's rearrange the equation to solve for V:

`(nxxRxxT)/P`

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

`V = 59.6 L`

Answer 2

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.