Michael S. answered 08/05/26
B.S. in Chemistry, Indiana University; Organic Chem Teaching Intern
About 2.6 atm on the gauge (3.54 atm absolute).
That note about gauge pressure is not a footnote — it is the entire problem. Gas laws require absolute pressure, and the tire gauge does not report it.
Step 1 — convert gauge to absolute
Pabs = Pgauge + Patm = 2.3 + 0.987 = 3.287 atm
A gauge reads zero in open air, so it is measuring how much the tire exceeds its surroundings. The gas inside does not know about that offset — it responds to the total pressure it actually exerts.
Step 2 — convert temperatures to kelvin
T1 = 20 + 273.15 = 293.15 K
T2 = 43 + 273.15 = 316.15 K
Celsius will not work here either. The ratio 43/20 = 2.15 would predict the pressure more than doubling; the true ratio is 316.15/293.15 = 1.078, a 7.8% rise. Kelvin is required because gas laws are proportionalities, and only an absolute scale makes ratios meaningful.
Step 3 — Gay-Lussac's law (volume and moles fixed, since a tire is rigid and sealed)
P1/T1 = P2/T2
P2 = (3.287 atm)(316.15 / 293.15) = 3.545 atm absolute
Step 4 — back to gauge, since that is what the question asks
Pgauge = 3.545 − 0.987 = 2.56 ≈ 2.6 atm
Why the conversion matters numerically
Skip it and apply the temperature ratio straight to the gauge reading: 2.3 × 1.078 = 2.48 atm. That is off by about 0.08 atm — a small-looking gap that is entirely an artifact of using the wrong pressure scale. Convert → solve → convert back, every time.
The practical version of this result: a 23 °C temperature rise added roughly 0.26 atm (about 3.8 psi) to the tires. This is why you check tire pressure when the tires are cold, and why pressure warnings often appear on the first cold morning of autumn — nothing leaked, the air just cooled.