Use the References to access important values if needed for this question. Tire pressure gauges are often calibrated in pounds per square inch. An automobile tire is inflated to a pressure of 28.6 psi. Express this pressure in atmospheres and in millimeters Hg. Hint: 1 atm = 760 mmHg = 14.7 psi Pressure = Pressure = Submit Answer Q Search J a atm mmHg Retry Entire Group 9 more group attempts remaining myhp e

Use the References to access important values if needed for this question. Tire pressure gauges are often calibrated in pounds per square inch. An automobile tire is inflated to a pressure of 28.6 psi. Express this pressure in atmospheres and in millimeters Hg. Hint: 1 atm = 760 mmHg = 14.7 psi Pressure = Pressure = Submit Answer Q Search J a atm mmHg Retry Entire Group 9 more group attempts remaining myhp e

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter5: Gases

Section: Chapter Questions

Problem 130E

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At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A 0.8765-g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The oxygen gas collected over water occupied 57.2 mL at a temperature of 22C and a pressure of 734 torr. Calculate the mass percent of NaClO3 in the original sample. (At 22C the vapor pressure of water is 19.8 torr.)
perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.
You have a gas, one of the three known phosphorus-fluorine compounds (PF3, PF3, and P2F4). To find out which, you have decided to measure its molar mass. (a) First, yon determine that the density of the gas is 5.60 g/L at a pressure of 0.971 atm and a temperature of 18.2 C. Calculate the molar mass and identify the compound. (b) To check the results from part (a), you decide to measure the molar mass based on the relative rales of effusion of the unknown gas and CO2. You find that CO2 effuses at a rate of 0.050 mol/min, whereas the unknown phosphorus fluoride effuses at a rate of 0.028 mol/min. Calculate the molar mass of the unknown gas based on these results.
93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
Carbon dioxide, CO2, was shown lo effuse through a porous plate at the rate of 0.033 mol/min. The same quantity of an unknown gas, 0.033 moles, is found to effuse through the same porous barrier in 104 seconds. Calculate the molar mass of the unknown gas.
A typical barometric pressure in Redding. California, is about 750 mm Hg. Calculate this pressure in atm and kPa.
5-56 The three main components of dry air and the percentage of each are nitrogen (78.08%), oxygen (20.95%), and argon (0.93%). (a) Calculate the partial pressure of each gas in a sample of dry air at 760 mm Hg. (b) Calculate the total pressure exerted by these three gases combined.
A mixture of chromium and zinc weighing 0.362 g was reacted with an excess of hydrochloric acid. After all the metals in the mixture reacted, 225 mL dry of hydrogen gas was collected at 27C and 750. torr. Determine the mass percent of Zn in the metal sample. [Zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen gas; chromium reacts with hydrochloric acid to produce chromium(III) chloride and hydrogen gas.]
5-34 A sample of 30.0 mL of krypton gas, Kr, is at 756 mm Hg and 25.0°C. What is the new volume if the pressure is decreased to 325 mm Hg and the temperature is decreased to-12.5°C?
A certain flexible weather balloon contains helium gas at a volume of 855 L. Initially, the balloon is at sea level where the temperature is 25C and the barometric pressure is 730 torr. The balloon then rises to an altitude of 6000 ft, where the pressure is 605 torr and the temperature is 15C. What is the change in volume of the balloon as it ascends from sea level to 6000 ft?
Ethanol, C2H5OH, is produced industrially from ethylene, C2H4, by the following sequence of reactions: 3C2H4+2H2SO4C2H5HSO4+( C 2 H 5)2SO4C2H5HSO4+( C 2 H 5)2SO4+3H2O3C2H5OH+2H2SO4 What volume of ethylene at STP is required to produce 1.000 metric ton (1000 kg) of ethanol if the overall yield of ethanol is 90.1%?
5-33 A certain quantity of helium gas is at a temperature of 27 °C and a pressure of 1.00 atm. What will the new temperature be if its volume is doubled at the same time that its pressure is decreased to one-half its original value?

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