A race car driver starts a race with his tires at 13.2 psi at a temperature of 25 C. What will the pressure in the tires be (in psi) when they heat up to 63 C?

Question

Chemistry

Halle Roberts

20 May, 06:36

A race car driver starts a race with his tires at 13.2 psi at a temperature of 25 C. What will the pressure in the tires be (in psi) when they heat up to 63 C?

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Answers (1)

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Bria · Answer 1

P₂ = 14.88 psi

Explanation:

Given dа ta:

Initial pressure of tires = 13.2 psi

Initial temperature = 25°C (25+273 = 298 K)

Final pressure in tires = ?

Final temperature = 63°C (63+273 = 336 K)

Solution:

According to Gay-Lussac Law,

The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.

Mathematical relationship:

P₁/T₁ = P₂/T₂

Now we will put the values in formula:

13.2 / 298 K = P₂/336 K

P₂ = 13.2 psi * 336 K / 298 K

P₂ = 4435.2 psi. K / 298 K

P₂ = 14.88 psi