A car tire has a recommended rating of 2.518 atm. While parked, the tire has at the temperature of11.00C, inflated to a volume of 10.4 L and with a pressure of 2.109 atm. When driving on a hot day, thetire warms to 62.0 Cand its volume expands to 10.9 Ld) Knowing the number of mols in the tire use the Ideal Gas law to calculate the final pressureat 62 C, is it the same as your answer in Ae) While parked (11 C) you inflated the tire to 2.38 atm assuming there is no temperaturechange what is the new volume of the tire?f) Once you finish your drive, the tire temperature is 62 oC, after 10 minutes of being parkedthe temperature of the tire is now 58°C assuming your tire volume does not change what isthe new pressure of the tire? (get the original pressure form C)

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Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter5: Gases

Section: Chapter Questions

Problem 26Q: Consider two different containers, each filled with 2 moles of Ne(g). One of the containers is rigid...

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Similar questions

The following figure shows three 1.00-L bulbs connected by valves. Each bulb contains argon gas with amounts proportional to the number of circles pictorially represented in the chamber. All three bulbs are maintained at the same temperature. Unless stated otherwise, assume that the valves connecting the bulbs are closed and seal the gases in their respective chambers. Assume also that the volume between each bulb is negligible. (a) Which bulb has the highest pressure? (b) If the pressure in bulb A is 0.500 atm, what is the pressure in bulb C? (c) If the pressure in bulb A is 0.500 atm, what is the total pressure? (d) If the pressure in bulb A is 0.500 arm, and the valve between bulbs A and B is opened, redraw the figure shown above to accurately represent the gas atoms in all three bulbs. What is P A+P B+P C? Compare your answer in part (d) to that in part (c). (e) Follow the instructions of part (d) but now open only the valve between bulbs B and C.
Shown below are three containers of an ideal gas (A, B, and C), each equipped with a movable piston (assume that atmospheric pressure is 1.0 atm). a How do the pressures in these containers compare? b Are all the gases at the same temperature? If not, compare the temperatures. c If you cooled each of the containers in an ice-water bath to 0.0C, describe how the volumes and pressures of the gases in these containers would compare.
A sample of a compound of xenon and fluorine was confined in a bulb with a pressure of 18 tor. Hydrogen was added to the bulb until the pressure was 72 torr. Passage of an electric spark through the mixture produced Xe and HF. After the HF was removed by reaction with solid KOH, the final pressure of xenon and unreacted hydrogen in the bulb was 36 torr. What is the empirical formula of the xenon fluoride in the original sample? (Note: Xenon fluorides contain only one xenon atom per molecule.)
A 1 007-g sample of an unknown gas exerts a pressure of 715 mm Hg in a 452-mL container at 23 C. What is the molai mass of the gas?
Consider two different containers, each filled with 2 moles of Ne(g). One of the containers is rigid and has constant volume. The other container is flexible (like a balloon) and is capable of changing its volume to keep the extemal pressure and internal pressure equal to each other. If you raise the temperature in both containers, what happens to the pressure and density of the gas inside each container? Assume a constant extemal pressure.

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