Answered: A tire is filled with air at 20 deg C… | bartleby

Related questions

Question

A tire is filled with air at 20 deg C and a gauge pressure of 220 kPa. If the tire reaches 50 deg C
(let's say in Death Valley in the summer), what fraction of the original air must be removed in
order for the gauge pressure to remain 220 kPa?

Expert Solution

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Blurred answer

Similar questions

A basketball is pressurized to a gauge pressure of PG = 55 kPa when at the surface of a swimming pool. (Patm = 101 kPa). The ball is then submerged in the pool of water which has a density ρ = 1000 kg/m3. Assume the ball does not change in mass, temperature, or volume as it is submerged. Calculate the absolute pressure inside the basketball in kPa when it is at the surface. Write an equation for the pressure difference ΔP between the inside and outside of the ball when it is submerged a distance y below the surface of the water. Solve the pressure equation for the depth (in meters) at which the pressure difference between the inside and outside of the ball will become zero. At this depth the pressure inside the basketball is the same as the pressure outside the ball.
(a) How many molecules are present in a sample of an ideal gas that occupies a volume of 1.90 cm³, is at a temperature of 20°C, and is at atmospheric pressure? molecules -11 (b) How many molecules of the gas are present if the volume and temperature are the same as in part (a), but the pressure is now 1.50 x 10¯ Pa (an extremely good vacuum)? molecules
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 39.0°C. (a) What is the tire pressure in pascals? 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? Pa
If 2.00 mol of nitrogen gas (N2) are placed in a cubic box, 34.0 cm on each side, at 2.50 atm of pressure, what is the rms speed of the nitrogen molecules? 730.13 * m/s
Step 1 (a) The ideal-gas equation describes each condition of the air in the tire. We will set up ratios in order to describe these changes. Dividing the equations PV = nRT in the initial and final states, we have PfVf Tf P¡Vi Ti Solving for the final pressure in the tire, gives Pf = = = which gives I Tf P(V)() P₁ Vf T₁ = (1.013 x 105 Pa) x 105 Pa. Note that the volume V¡ cancels out of the equation. = Vf Po = Pr (V ( ) ( ) Pd Pf Vi V₁ Step 2 (b) After the car is driven, the temperature and volume of air in the tire have changed. Let Td be the temperature and Vd be the volume of air in the tire. We have PdVd Td PfVf Tf' x 105 Pa 273 + 273 + Vf Vf Again we see that the volume Vf cancels out of the equation. °C K °℃ K = x 105 Pa.
A large cylindrical tank contains 0.760 m3 of nitrogen gas at 20.0 ∘C and 1.45×105 Pa (absolute pressure). The tank has a tight-fitting piston that allows the volume to be changed. What will be the pressure if the volume is decreased to 0.410 m3 and the temperature is increased to 159 ∘C? Express your answer in pascals.
The density of helium gas at 0.0◦C is0.16 kg/m3kg/m3. The temperature is thenraised to 102 ◦C, but the pressure is kept constant.Assuming that helium is an ideal gas, calculate the new density of the gas.Answer in units of kg/m3.
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.