How many grams of air (M = 29 g/mol) must be pumped into an automobile tire if it is to have a gauge pressure of 33 psi? (Assume the volume of the tire is 5,800 cm3 and its temperature is 21 degrees C)
How many grams of air (M = 29 g/mol) must be pumped into an automobile tire...
Air is pumped into a bicycle tire. The air initially in the tire has a volume of 2695 cm3, a temperature of 22.0° C, and a gauge pressure of 2.00 atm. How many molecules of air must be pumped into the tire in order to raise the gauge pressure to 5.00 atm? Assume that the volume and temperature of the air inside the tire are approximately constant
Air is pumped into a bicycle tire. The 14 moles of air initially in the tire have a gauge pressure of 3 atm. How many moles of air must be pumped into the tire in order to raise the gauge pressure to 4 atm? Assume that the volume and temperature of the air inside the tire are approximately constant.
Review Part A An automobile tire has a volume of 2.50x10 m At a temperature of 299 K the absolute pressure in the tire is 215 kPa How many moles of air must be pumped into the tire to increase its pressure to 271 kPa, given that the temperature and volume of the tire remain constant? VO A An mol Request Answer Submit Next Provide Feedback
when the temperature of an automobile tire is 20 degrees c, the pressure in the tire reads 29 psi on a tire gauge. (the gauge measures the difference between the pressures inside and outside the tire.) what is rhe pressure when the tire heats up to 39 degrees c while driving? you may assume that the volume of the tire remains the same and that the atomspheric pressure is a steady 14 psi.
An automobile tire has a volume of 1.90×10−2 m3 . At a temperature of 294 K the absolute pressure in the tire is 214 kPa . How many moles of air must be pumped into the tire to increase its pressure to 265 kPa , given that the temperature and volume of the tire remain constant?
An automobile tire has a maximum rating of 38.0 psi (gauge pressure). The tire is inflated (while cold) to a volume of 11.8 L and a gauge pressure of 36.0 psi at a temperature of 12.0 °C. Driving on a hot day, the tire warms to 65.0 °C and its volume expands to 12.2 L. Does the pressure in the tire exceed its maximum rating? (Note: the gauge pressure is the difference between the total pressure and atmospheric pressure. In...
1. The pressure in an automobile tire depends on the temperature of the air in the tire. When the air temperature is 25C, the pressure gage reads 210 kPa. If the volume of the tire is 0.025 m determine the pressure rise in the tire when the air temperature in the tire rises to S0C. Also, determine the amount of air that must be bled off to restore pressure to its original value at this temperature. Assume the atmospheric pressure...
How many moles of gas must be forced into a 5.4 L tire to give it a gauge pressure of 30.6 psi at 21 ∘C? The gauge pressure is relative to atmospheric pressure. Assume that atmospheric pressure is 14.9 psi so that the total pressure in the tire is 45.5 psi . Express your answer using two significant figures.
An automobile tire has a maximum rating of 38.0 psi (gauge pressure). Part A The tire is inflated (while cold) to a volume of 11.8 L and a gauge pressure of 36.0 psi (Note: The gauge pressure is the difference between the total pressure and atmospheric pressure. In this case, assume that atmospheric pressure is 14.7 psi.) at a temperature of 12.0°C. While driving on a hot day, the tire warms to 65.0°C and its volume expands to 12.2 L. What is the total...
An automobile tire has a volume of 1.61 x 10-2 m3 and contains air at a gauge pressure (pressure above atmospheric pressure) of 167 kPa when the temperature is 0.00°C. What is the gauge pressure of the air in the tires when its temperature rises to 28.6°C and its volume increases to 1.69 x 10-2 m3? Assume atmospheric pressure is 1.01 x 105 Pa.