At the end of a warm autumn day, you measure the air pressure in your car's tires and write down their pressure as 2.41 × 105 Pa (about 35 psi) when the outside temperature is 23°C. It cools down quite a bit overnight to -5°C. If you were to measure the air pressure in the tire on that cool morning, what pressure would you measure? Assume that you can ignore the change in the volume of the tire and that no air is released from the tire overnight.

An automobile tire is inflated with air originally at 10.0°C and normal atmospheric pressure. During the process, the air is compressed to 27.0% of its original volume and the temperature is increased to 38.0°C. (a) What is the tire pressure in pascals? Use the ideal gas law to find the pressure inside the tire from its volume and temperature. Pa(b) After the car is driven at high speed, the tire's air temperature rises to 85.0°C and the tire's interior volume increases by 3.00%. What is the new tire pressure (absolute) in pascals?

If gas pressure (absolute value) for an ideal gas is held constant, the relationship between gas temperature and volume is direct inverse of the form y = mx + c O parabolic

The gauge pressure in your car tires is 2.55 × 105 Pa at a temperature of 35.0°C when you drive it onto a ferry boat to Alaska. What is the gauge pressure of the tires, in pascals, later when the temperature has dropped to -40.0°C? Assume the volume of each tire does not change.

A balloon is filled with helium gas at atmospheric pressure (1 atm) until its volume is 800 m³. The helium gas is then transferred to cylinders that have a volume of 2.3 m³ at a pres- sure of 13.3 atm. Calculate the number of cylinders used. Assume that the temperature of the helium gas remains constant. (1 atm = 1.013 × 105 Pa).

n = 3.9 moles of an ideal gas are pumped into a chamber of volume V = 0.135 m3   50% Part (a)  The initial pressure of the gas is 1 atm. What is the initial temperature (in K) of the gas?  T = 421.76T = 421.8     ✔ Correct!     50% Part (b)  The pressure of the gas is increased to 10 atm. Now what is the temperature (in K) of the gas?

The number density of gas atoms at a certain location in the space above our planet is about 0.75 × 10!1 m²³, and the pressure is 2.9 x 10- 10 Pa in this region. What is the temperature in this region, in degrees Celsius? T =

Suppose you have a closed rigid container of air at 20 Celsius on the surface of the Earth. We increase the temperature of the container to 77, leaving it closed, and read a pressure gauge attached to the container.  Initially the reading was 101 KPa (kilopascals, or 1000 N/m2).  What is the new reading? Give your answer in KPa.

An ideal gas at 7°C is in a spherical flexible container having a radius of 1.04 cm. The gas is heated at constant pressure to 88°C. Determine the radius of the spherical container after the gas is heated. [Volume of a sphere = (4/3)?r3.]