A certain automobile tire has a volume of 0.0185 m³. If the absolute (or total) pressure in the tire is 500 kPa and the temperature is 298 K, how many molecules are there inside the tire? (R = 8.31 J/mol ∙ K, N_A = 6.022 x 10²³ molecules/mol) A) 2.25 × 10²³ molecules B) 2.25 × 10²⁴ molecules C) 3.25 × 10²³ molecules D) 3.25 × 10²⁴ molecules E) 3.25 × 10²⁵ molecules

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Quizplus · Accepted Answer

Using the ideal gas law PV = nRT, we can solve for n (number of moles): n = PV / RT. Substituting the given values, we find n = (500,000 Pa)(0.0185 m³) / (8.31 J/mol∙K)(298 K). Then, multiply n by Avogadro's number (N_A) to find the number of molecules: n × 6.022 × 10²³ molecules/mol. This calculation results in approximately 2.25 × 10²⁴ molecules.

A Certain Automobile Tire Has a Volume of 0