What final temperature (∘c) is required for the pressure inside an automobile tire to increase from 2.19 atm at 0 ∘c to 2.37 atm, assuming the volume remains constant?

Question

Chemistry

Rodolfo Mckinney

5 September, 18:10

What final temperature (∘c) is required for the pressure inside an automobile tire to increase from 2.19 atm at 0 ∘c to 2.37 atm, assuming the volume remains constant?

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Khloe Scott · Answer 1

22.45 c

The ideal gas law is PV = nRT where P = pressure V = volume n = number of moles R = ideal gas constant T = absolute temperature Since converting from 0 centigrade to kelvin, we get an absolute temperature of 273.15 K. Because the values of P, n, and R are all remaining constant, we can simplify the equation to a simple ratio of pressure vs temperature. So P1/P2 = T1/T2 Cross multiply P1*T2 = P2*T1 And divide by P1 T2 = P2*T1/P1 Substitute the known values and calculate T2 = P2*T1/P1 T2 = 295.6006849 So the final temperature is 295.6 K, which we need to convert to C by subtracting 273.15 295.6 - 273.15 = 22.45068493 So the answer to two decimal places is 22.45âc