How many moles of gas are present when you collect 35.83 mL of the gas over water at 25.3°C and 0.97 atm?

Use Ideal Gas equation since values are given in Pressure (P), Volume (V), Temperature (T).

P V = n R T; n = PV / RT

You can't use 1 mole = 22.4 L equation. Temperature and pressure values are not standard. (1 atm, 0

To choose the value of R (gas constant), check out the units of other values in the equation. They are in atm, liter, kelvin, and mole. So, its value is 0.082 L atm / K mol.

P = 0.97 atm

V = 35.83 * 10 ⁻³ L (conversion from ml to, just multiplied by 10 ⁻³)

R = 0.082 L atm / K mol

T = (25.3 + 273) K (recall Kelvin = Celcius + 273; K = °C + 273)

Substitute values into equation of n = PV / RT

n = (0.97 atm) (35.83 * 10 ⁻³ L) / (0.082 L atm / K mol) (298.3 K) = 0.014 mole

The answer is 0.014 mole