The formula shown is correct.
The temperature was correctly converted to Kelvin as well.
You need to convert the psi to atm.
Psi to atm formula = Total pressure/ atmospheric pressure
48.4/14.8 = 3.2703
14.8 atm x 5.0 = n x 0.0821 x 301K
74 = 24.7121
74/24.71 = 2.99 mol
(please dislike if this is wrong.)
How many moles of gas must be forced into a 5.0 L tire to give it a gauge pressure of 33.6 psi at 28 ∘C? The gauge pressure is relative to atmospheric pressure. Assume that atmospheric pressure is 14.8 psi so that the total pressure in the tire is 48.4 psi .
PV = nRT
48.4 x 5.0 = n x .0821 x 301K
9.79 mol
1 answer