How many moles of gas must be forced into a 4.8L tire to give it a gauge pressure of 32.6psi at 26∘C? The gaug?
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Update:How many moles of gas must be forced into a 4.8L tire to give it a gauge pressure of 32.6psi at 26∘C? The gauge pressure is relative to atmospheric pressure. Assume that atmospheric pressure is 14.8psi so that the total pressure in the tire is 47.4psi .
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p = 326,8 kPa , T = 299 K, R = 8,314, V = 4,8*10^-3 m^3
pV = nRT
n = pV / RT = 0,631 moles
Hello princesse: Apply the Ideal Gas Law:
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nf = PV/RT
nf = ( 47.4 / 14.7 ) ( 4.8 ) / ( 0.08205 ) ( 299.2 ) = 0.6304 gmol = final moles
ni = ( 14.8 /14.7 ) ( 4.8 ) / ( 0.08205 ) ( 299.2 ) = 0.1969 gmol = initial moles
na = nf - ni = 0.6304 - 0.1969 = 0.4335 gmol added to tire <----------------------------------