On a spring morning (20.^$\circ$C) you fill your tires to a pressure of 2.25 atmospheres. As you ride along, the tire heats up to 45^$\circ$C from the friction on the road. What is the pressure in your tires now in units of atmospheres

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Quizplus · Accepted Answer

To solve this problem, we can use the ideal gas law in the form of $P_1/T_1 = P_2/T_2$, where $P$ is pressure, $T$ is temperature in Kelvin, and the subscripts 1 and 2 refer to the initial and final states, respectively. First, convert the temperatures from Celsius to Kelvin by adding 273.15. The initial temperature is $20 + 273.15 = 293.15$ K, and the final temperature is $45 + 273.15 = 318.15$ K. The initial pressure $P_1$ is 2.25 atmospheres. We solve for $P_2$ as follows:$$P_2 = P_1 \times \frac{T_2}{T_1} = 2.25 \times \frac{318.15}{293.15}$$$$P_2 \approx 2.25 \times 1.085 = 2.441 atmospheres$$Since 2.441 atmospheres is not one of the given options, the correct answer is E) None of the above.

On a Spring Morning (20 ∘\circ∘ C) You Fill Your Tires to a Pressure of 2

On a Spring Morning (20 $\circ$ C) You Fill Your Tires to a Pressure of 2