# A sample of Hydrogen gas, H2,

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

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

pts On a very cold day, you notice that your tires look a bitdeflated 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 pressuremonitoring 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 Alaskawhere the temperature drops to 20 °F. As you arrived in Alaska, younoticed that the tire pressure monitoring system alert light isilluminated. Why did this happen? a) as temperature decreases, gasmolecules lose kinetic energy and the volume of gas is reduced thusreducing the overall pressure in the tire which results in the TPMSto become activated b) as temperature decreases, gas molecules gainkinetic energy and the volume of gas is reduced thus reducing theoverall pressure in the tire which results in the TPMS to becomeactivated c) as temperature decreases, gas molecules lose kineticenergy and the volume of gas increases thus reducing the overallpressure in the tire which results in the TPMS to becomeactivated

Question 91 pts On a hot summer day, you notice that a bag ofchips left in your vehicle has inflated. Why did this happen?(Outcome # 6) (DOK 3) a) as temperature increases, gas moleculesgain kinetic energy and the volume of gas decreases inside the bagof chips b) as temperature increases, gas molecules lose kineticenergy and the volume of gas increases inside the bag of chips c)as temperature increases, gas molecules gain kinetic energy and thevolume 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 thesame container. What is the total pressure in the container? a)2.07 atm b) 1.94 atm c) 0,135 atm

Answer:

1) A sample of Hydrogen gas, H2, hasa volume of 8.56 L at a temperature of 0oC and a pressure of1.5atm. Calculate the number of moles of hydrogen gas in thissample.

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

**Answer: 0.57mol**

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2) Question 5Our next lab involvesdetermining the partial pressure of an evolved gas in the processof a chemical reaction. If the atmospheric pressure is found to be75.4 cm Hg, and the partial pressure of water is known to be (foundin a reference table) 21 torr, what is the partial pressure of ourevolved 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: 0.964atm**

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3) On a very cold day, you noticethat your tires look a bit deflated than warmer days. Thisobservation can be explained by _____. Boyles Law Charles Law IdealGas Law

**Answer: CharlesLaw**

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

**Answer: as temperaturedecreases, gas molecules lose kinetic energy and the volume of gasincreases thus reducing the overall pressure in the tire whichresults in the TPMS to become activated**. PV = constant

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5) Question 91 pts On a hot summerday, you notice that a bag of chips left in your vehicle hasinflated. Why did this happen? (Outcome # 6) (DOK 3) a) astemperature increases, gas molecules gain kinetic energy and thevolume of gas decreases inside the bag of chips b) as temperatureincreases, gas molecules lose kinetic energy and the volume of gasincreases inside the bag of chips c) as temperature increases, gasmolecules gain kinetic energy and the volume of gas increasesinside the bag of chips

**Answer: a) as temperatureincreases, gas molecules gain kinetic energy and the volume of gasdecreases inside the bag of chips.** Again here volumedecreases 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 totalpressure 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) 2.07atm**

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