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CHMLL 130 MCCRSCC Exploring Gas Behavior Moles and Volume of A Gas Lab Report

CHMLL 130 MCCRSCC Exploring Gas Behavior Moles and Volume of A Gas Lab Report

Question Description

I’m working on a chemistry question and need guidance to help me learn.

C. Part I Follow-Up Questions (Show all calculations with units on each number and the final answer rounded to the correct significant figures for full credit.)

  1. Calculate balloon volume for each balloon at maximum inflation from the circumference data. (You will have to assume that the balloon was a perfect sphere.) To calculate balloon volume, first find the radius (in cm) of the balloon by using the formula C = 2?r. Then, use the radius’ value in the formula V = (4/3)?r3 to calculate volume (in cm3). Show all your work, place units on all numbers (even those within the calculations), and express your answers with appropriate sig figs. (12 pts)
  2. Calculate the experimental value for the number of moles of CO2 in each balloon at maximum inflation using the formula PV = nRT. Use the volume you calculated in Question 1 at maximum inflation and recall that the gas constant R is 8.206 x 10-2 L atm/mol K. To find the temperature, look at your home thermostat. To find the pressure, use the internet to access the National Weather Service internet website. It will give you the pressure at your location on the day you perform the experiment. [Note: It is essential that your pressure as measured by the barometer be converted from the unit of inHg (inches of mercury) to atm, temperature from oF to K, and volume from cm3 to L before using the ideal gas law and the ideal gas constant.] (12 pts)
  3. Calculate the theoretical value for the number of moles of CO2 that should have been produced in each balloonassuming that 1.45 g of NaHCO3 is present in an antacid tablet. Use stoichiometry (a mole ratio conversion must be present) to find your answers (there should be three: one answer for each balloon). (6 pts)

The balanced chemical equation for this reaction is:

H3C6H5O7(aq) + 3 NaHCO3(aq) ? 3 CO2(g) + 3 H2O(l) + Na3C6H5O7(aq)

4.What is the percent error between the experimental value of moles of CO2 (from Question 2) and the theoretical value of moles of CO2 (from Question 3) for each balloon? (3 pts)

5.How do your experimental and theoretical values compare (discuss percent error from Question 4)? Explain any discrepancies and list TWO sources of error (“human error” and “calculator error” are unacceptable responses; your sources of error should be based on potential flaws in the experimental procedure or design). (6 pts)

6.Graph balloon volume versus the number of tablets used in a line graph. Since the independent variable in this experiment was the number of tablets used, that variable should be plotted on the horizontal axis. The dependent variable was the volume of the balloon; that variable should be plotted on the vertical axis. Be sure to use MS Excel or Graphical Analysis to create your graph and then copy/paste it here. Be sure to include a title for the graph, as well as labels with appropriate units on each axis. (6 pts)

7.Describe the relationship between the number of tablets in the balloon and the volume of the balloon as shown in your graph. (4 pts)

C. Part II Follow-Up Questions (Show all calculations with units on each number and the final answer rounded to the correct significant figures for full credit.)

  1. Calculate the balloon volume of balloon #1 at both room temperature and at the high temperature using average circumference data. (You will have to assume that the balloon was a perfect sphere.) To calculate balloon volume, first find the radius (in cm) of the balloon by using the formula C = 2?r. Then, use the radius’ value in the formula V = (4/3) ?r3 to calculate volume (in cm3). Show all your work, place units on all numbers (even those within the calculations), and express your answers with appropriate sig figs. (8 pts)
  2. What happened to the volume of balloon #1 as its temperature increased? Use numerical data from Question 8 to support your response. (4 pts)
  3. Explain the results from Part II. Your explanation must discuss the behavior of gas particles. (6 pts)
  4. Which gas law does Part II of the lab demonstrate? How do you know? What is the equation associated with this law? (3 pts)
  5. Using the law from your answer to Question 11, explain what would happen to a balloon if it were placed in a freezer for 15 minutes. Support your answer with data from the lab and/or content from the lab’s Background Information. (4 pts)

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