The car owner accidentally fills the tires to a pressure of 45 psi at 70 °F. The tire pressure should never exceed a pressure of 48 psi, otherwise the tires may burst. However, during driving the tires may heat up to 120 °F. Calculate the tire pressure at 120 °F, assuming ideal gas behavior and that the volume of the tire is constant. Will the car tires burst if they heat up to 120 °F?

The car owner accidentally fills the tires to a pressure of 45 psi at 70 °F. The tire pressure should never exceed a pressure of 48 psi, otherwise the tires may burst. However, during driving the tires may heat up to 120 °F. Calculate the tire pressure at 120 °F, assuming ideal gas behavior and that the volume of the tire is constant. Will the car tires burst if they heat up to 120 °F?

Similar questions

EC1q7 May I please have assistance with this question? thank you
Amanda discovers that the gauge pressure in her car tires is 2.50 ×105 Pa at a temperature of 35.0oC. The average volume of a single tire at that temperature is 10.0 L. 1.) Find how many moles of gas (air) are in one of Steve’s tires. 2.) Later Amanda travels to a place where the temperature is –40.0oF. She notices that the tires are looking low and estimates that each tire has lost approximately 1.0 L of its volume. What is the gauge pressure in the tire now?
Two evacuated bulbs are connected by a tube of negligible volume. The volume of one of the bulbs is twice that of the other. The larger volume bulb is placed in a 200K Isother constant-temperature bath and the other in a 300K bath, and then 1.00mol of an ideal me gas is injected into the system. Find the final number of moles of gas in each bulb.
Air is pumped into a bicycle tire. The 42 moles of air initially in the tire have a gauge pressure of 4 atm. How many moles of air must be pumped into the tire in order to raise the gauge pressure to 8 atm? Assume that the volume and temperature of the air inside the tire are approximately constant.
Three moles of an ideal gas at 135C and 0.5 atm is allowed to expand 1 atm at a constant pressure to a volume twice as large. What is the new temperature?
5kg on it which can slide up and A cylinder with an ideal gas has a piston of mass m = down and does not permit the gas to escape. The inner radius of the cylinder is r = 6cm, The top of the piston is open to atmospheric pressure. The entire system is initially in thermal equilibrium with the environment, which is at 20°C and the height of the piston h = 10cm. If the temperature of the gas inside then is raised to 100°C, what is the final height of the piston? A 20 cm В 50 cm C 12.7 cm D 25.4 cm 18 cm Open to outside air, pressure po Piston, mass m Ideal- gas
A) A rigid tank contains 1.60 moles of helium, which can be treated as an ideal gas, at a pressure of 28.0 atm. While the tank and gas maintain a constant volume and temperature, a number of moles are removed from the tank, reducing the pressure to 5.00 atm. How many moles are removed? B) What If? In a separate experiment beginning from the same initial conditions, including a temperature Ti of 25.0°C, half the number of moles found in part (a) are withdrawn while the temperature is allowed to vary and the pressure undergoes the same change from 28.0 atm to 5.00 atm. What is the final temperature (in °C) of the gas?
(a) What is the gauge pressure in a 25.0oC car tire containing 3.60 mol of gas in a 30.0 L volume? (b) What will its gauge pressure be if you add 1.00 L of gas originally at atmospheric pressure and 25.0oC? Assume the temperature returns to 25.0oC and the volume remains constant.