Question

Question #e66a1

Answer 1

Under those conditions for temperature and pressure, 0.3 moles of methane would occupy that volume.

Explanation:

You have all the information you need to solve for the number of moles of methane that would occupy 4.3 L at a temperature of 400 K and a pressure of 2 atm.

Your tool of choice will be the ideal gas law equation

`PV = nRT`, where

`P` - pressure;
`V` - the volume the gas occupies;
`n` - the number of moles of gas;
`R` - the ideal gas constant, equal to `0.082("atm" * "L")/("mol" * "L")`
`T` - the temperature of the gas.

Plug your values into the equation and solve for `n`

`PV = nRT => n = (PV)/(RT)`

`n = (2cancel("atm") * 4.3cancel("L"))/(0.082(cancel("atm") * cancel("L"))/("mol" * cancel("K")) * 400cancel("K"))`

`n = "0.262 moles"`

Rounded to one sig fig, the number of sig figs you gave for the temperature of the gas, the answer will be

`n = color(green)("0.3 moles")`