CHE-121 WA6.docx - Name Jesus Espinosa College ID 0441797 Thomas Edison State University General Chemistry I with Labs(CHE-121 Section no OL009 Semester

# CHE-121 WA6.docx - Name Jesus Espinosa College ID 0441797...

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Name: Jesus Espinosa College ID: 0441797 Thomas Edison State University General Chemistry I with Labs (CHE-121) Section no.: OL009 Semester and year: June 2018 Written Assignment 6: Gases Answer all assigned questions and problems, and show all work. 1. A gas occupying a volume of 725 mL at a pressure of 0.970 atm is allowed to expand at constant temperature until its pressure reaches 0.541 atm. What is its final volume? (5 points) P 1 V 1 =P 2 V 2 P 1 =0.970atm V 1 =725mL P 2 =0.541 atm V 2 = x V 2 = P 1 V 1 P 2 = 0.970 atm (725mL)/ 0.541 atm = 1.30 x 10 3 mL (Reference: Chang 5.19) 2. The volume of a gas is 5.80 L, measured at 1.00 atm. What is the pressure of the gas in mmHg if the volume is changed to 9.65 L? (The temperature remains constant.) (5 points) 1atm = 760 mm Hg P 1 V 1 =P 2 V 2 P 1 = 760 mm Hg V 1 =5.8L P 2 = x V 2 = 9.65L P 2 = P 1 V 1 V 2 = 760 mmHg ( 5.8 L ) 9.65 L = 456.788 mm Hg (Reference: Chang 5.21) 3. Why is the density of a gas much lower than that of a liquid or solid under atmospheric conditions? What units are normally used to express the density of gases? (5 points) The forces of attraction between gas molecules are weaker than those in liquids and solids. This allows for the random movement of gas molecules independent of each other. Under atmospheric conditions this allows for gases to expand into larger volumes than a liquid or solid could occupy. Density = mass/volume. Mass is constant, volume increases, density decreases. We use units of grams per liter, g/L.
(Reference: Chang 5.30) 4. A sample of nitrogen gas kept in a container of volume 2.3 L and at a temperature of

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