The gauge pressure in your car tires is 2.50 ×10^5 N / m^2 at a temperature of 35.0^∘ C when you

step 1 So here we can use the ideal gas law. The pressure times the volume would be equal to n the numb

The gauge pressure in your car tires is 2.50 ×10^5 N / m^2...

The gauge pressure in your car tires is $2.50 \times 10^{5} \mathrm{N} / \mathrm{m}^{2}$ at a temperature of $35.0^{\circ} \mathrm{C}$ when you drive it onto a ferry boat to Alaska. What is their gauge pressure later, when their temperature has dropped to $-40.0^{\circ} \mathrm{C} ?$

Key Concepts

Ideal Gas Law

The ideal gas law, expressed as PV = nRT, relates the pressure (P), volume (V), number of moles of gas (n), temperature (T), and the universal gas constant (R). In situations where the volume of a container is fixed, changes in the absolute temperature result in proportional changes in the pressure, making it a key principle in understanding how temperature variations affect gas pressure.

Temperature Conversion

Temperature conversion, particularly from Celsius to Kelvin, is fundamental when working with gas laws such as the ideal gas law. Since these laws require temperature to be measured on an absolute scale, converting Celsius to Kelvin by adding 273.15 ensures that the proportional relationships between temperature and pressure (or volume) are accurately maintained.

Gauge Pressure

Gauge pressure represents the pressure in a system measured relative to the ambient atmospheric pressure. It is the difference between the absolute pressure inside a container, such as a tire, and the atmospheric pressure outside. This concept is important in practical applications where instruments display pressure readings that do not include the contribution of atmospheric pressure.

Absolute Pressure

Absolute pressure is the total pressure exerted within a system, including the atmospheric pressure. It is necessary to consider absolute pressure in theoretical calculations, especially when applying the ideal gas law, as it provides the complete picture of the pressure exerted by the gas particles.

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