You just calibrated a constant volume gas thermometer. The pressure of the gas inside the thermometer is 240.0 kPa when the thermometer is in contact with boiling water. The boiling water is under regular atmospheric pressure. What is the temperature of the thermometer, when it reads a pressure of 431.0 kPa?

396.97°C

Explanation:

Charles' Law explains that at constant volume, the pressure of an ideal gas is directly proportional to its temperature (in Kelvin).

P₁ ∝ T₁

P₁ = kT₁

k = constant of proportionality

(P₁/T₁) = (P₂/T₂)

P₁ = 240.0 kPa

T₁ = Boiling point of water = 100°C = 373.15 K

P₂ = 431.0 kPa

T₂ = ?

(240/373.15) = (431/T₂)

T₂ = (431 × 373.15) ÷ 240

T₂ = 670.12 K

T₂ = 396.97°C

Hope this Helps!!!

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explanation: