Question

A sample of Hydrogen gas, H2, has a volume of 8.56 L at a temperature of 0oC and a pressure of 1.5atm. Calculate the number of moles of hydrogen gas in this sample.

Question 5Our next lab involves determining the partial pressure of an evolved gas in the process of a chemical reaction. If the atmospheric pressure is found to be 75.4 cm Hg, and the partial pressure of water is known to be (found in a reference table) 21 torr, what is the partial pressure of our evolved gas, in atm? 1.02 atm 0.992 atm 0.964 atm

pts On a very cold day, you notice that your tires look a bit deflated than warmer days. This observation can be explained by _____. Boyles Law Charles Law Ideal Gas Law

Question 81 pts Suppose your car is equipped with tire pressure monitoring system (TPMS) and the tire pressure is 34.0 psi on a 98 °F day in California. You decided to take a road trip to Alaska where the temperature drops to 20 °F. As you arrived in Alaska, you noticed that the tire pressure monitoring system alert light is illuminated. Why did this happen? a) as temperature decreases, gas molecules lose kinetic energy and the volume of gas is reduced thus reducing the overall pressure in the tire which results in the TPMS to become activated b) as temperature decreases, gas molecules gain kinetic energy and the volume of gas is reduced thus reducing the overall pressure in the tire which results in the TPMS to become activated c) as temperature decreases, gas molecules lose kinetic energy and the volume of gas increases thus reducing the overall pressure in the tire which results in the TPMS to become activated

Question 91 pts On a hot summer day, you notice that a bag of chips left in your vehicle has inflated. Why did this happen? (Outcome # 6) (DOK 3) a) as temperature increases, gas molecules gain kinetic energy and the volume of gas decreases inside the bag of chips b) as temperature increases, gas molecules lose kinetic energy and the volume of gas increases inside the bag of chips c) as temperature increases, gas molecules gain kinetic energy and the volume of gas increases inside the bag of chips

Question 101 pts Oxygen gas (PO2 = 1.10 atm), nitrogen gas (PN2 = 0.840 atm), and carbon dioxide gas (PCO2 = 0.125 atm) occupy the same container. What is the total pressure in the container? a) 2.07 atm b) 1.94 atm c) 0,135 atm

Answer 1

1) A sample of Hydrogen gas, H2, has a volume of 8.56 L at a temperature of 0oC and a pressure of 1.5atm. Calculate the number of moles of hydrogen gas in this sample.

PV = nRT ==> n = PV/RT = [1.5 atm x 8.56 L] / [0.082057 L.atm/mol.K x 273 K] = 0.5732 mol

Answer: 0.57 mol

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2) Question 5Our next lab involves determining the partial pressure of an evolved gas in the process of a chemical reaction. If the atmospheric pressure is found to be 75.4 cm Hg, and the partial pressure of water is known to be (found in a reference table) 21 torr, what is the partial pressure of our evolved gas, in atm? 1.02 atm 0.992 atm 0.964 atm

Ptotal = Pgas + Pwater; 75.4 cmHg = 754 mm / 760 = 0.9921 atm; 21 torr = 0.0276316 atm

Pgas = Ptotal -Pwater = 0.09921 - 0.0276316 = 0.964 atm

Answer: 0.964 atm

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3) On a very cold day, you notice that your tires look a bit deflated than warmer days. This observation can be explained by _____. Boyles Law Charles Law Ideal Gas Law

Answer: Charles Law

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4) Question 81 pts Suppose your car is equipped with tire pressure monitoring system (TPMS) and the tire pressure is 34.0 psi on a 98 °F day in California. You decided to take a road trip to Alaska where the temperature drops to 20 °F. As you arrived in Alaska, you noticed that the tire pressure monitoring system alert light is illuminated. Why did this happen? a) as temperature decreases, gas molecules lose kinetic energy and the volume of gas is reduced thus reducing the overall pressure in the tire which results in the TPMS to become activated b) as temperature decreases, gas molecules gain kinetic energy and the volume of gas is reduced thus reducing the overall pressure in the tire which results in the TPMS to become activated c) as temperature decreases, gas molecules lose kinetic energy and the volume of gas increases thus reducing the overall pressure in the tire which results in the TPMS to become activated

Answer: as temperature decreases, gas molecules lose kinetic energy and the volume of gas increases thus reducing the overall pressure in the tire which results in the TPMS to become activated. PV = constant

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5) Question 91 pts On a hot summer day, you notice that a bag of chips left in your vehicle has inflated. Why did this happen? (Outcome # 6) (DOK 3) a) as temperature increases, gas molecules gain kinetic energy and the volume of gas decreases inside the bag of chips b) as temperature increases, gas molecules lose kinetic energy and the volume of gas increases inside the bag of chips c) as temperature increases, gas molecules gain kinetic energy and the volume of gas increases inside the bag of chips

Answer: a) as temperature increases, gas molecules gain kinetic energy and the volume of gas decreases inside the bag of chips. Again here volume decreases means pressure increases.

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6) Question 101 pts Oxygen gas (PO2 = 1.10 atm), nitrogen gas (PN2 = 0.840 atm), and carbon dioxide gas (PCO2 = 0.125 atm) occupy the same container. What is the total pressure in the container? a) 2.07 atm b) 1.94 atm c) 0,135 atm

Dalton's law P total = PO2+PN2+PCO2 = 1.10 + 0.840 + 0.125 = 2.065 ~ 2.07 atm

Answer: a) 2.07 atm

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