Question

How many grams of O2 gas are in a 3700 mL container at a pressure of 775 mmHg at 33oC?

Answer 1

Answer:

4.8 grams

Explanation:

Use PV=nRT

P: 775 mmHg (divide by 760 mmHg to get atm)  -> 1.02 atm

V: 3700 mL (divide by 1000 to get L)  -> 3.7L

n: ?

R: (a constant) 0.0821L * atm/k *mol

T: 33 C (add 273 to get K)  -> 306K

Move equation so n is on the side: PV/RT = n. Plug the numbers into the equation.

$\frac{1.02atm * 3.7L }{306K} * \frac{K * mol}{0.0821L *atm} = 0.15 mol$

Then, convert moles to grams using the molar mass of O2 which is 32g/mol.

$0.15 mol * \frac{32g}{mol}$= 4.8g