# How much gas is produced?

Topics: Gas, Pressure, Ideal gas law Pages: 7 (668 words) Published: December 2, 2013
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How Much Gas is Produced?
Julie Dang
June 23, 2013

Purpose
The Company ABC Chemical has asked our group to investigate the gas production from a number of various chemical reactions. The company would like us to measure the amount of product we get when we measure the amount of gas from two reactions. We will then compare our data to the predicted amount which will we will calculate based of the Law of conservation of Mass and Ideal Gas Laws.

Methods

Materials
Thermometer
CaCO3
Kim Wipes
1 M HCl (aq)
Mg Ribbon
Quantitative balance
Pressure sensor
GLX Machine
Syringe with white connectors
Tygon Tubing
125 mL flask with one-hole stopper

Procedure

Record the Temperature and convert into K
Determine the volume of the Flask and Tygon Tubing you will be using Connect the Pressure sensor to the GLX Machine and then connect the Tygon Tubing to the Pressure Sensor. Weigh the Mass of the Mg Ribbon and The CaCo3 and wrap it into a Kim Wipe. You should weigh out 0.7 g of Mg and 0.3 g of CaCO3 Add at least 16mL of 1.0 M HCl to the Erlenmeyer Flask. More than 16 mL would be better. Hold the flask sideways and place Kim Wipe with your solid wrapped inside the neck of the flask. Put the stopper in place and start the GLX Machine. After 10 seconds tilt the flask in upright position. Stir the flask and products inside and keep hands over the stopper to prevent the stopper from popping off. Once the gas stays at a steady rate or declines, stop the GLX Machine Data

Trial #1
Trial #2
Trial #3
Trial #1
Trial #2
Trial #3
Temperature
296.65
2296.65
296.65
296.65
296.65
296.65
Mass of Solid
0.07
0.079
0.073
0.034
0.03
0.033
Volume of HCl
16.7
16.2
16.9
16.3
16.9
16.3
141.8
141.8
141.8
141.8
141.8
141.8
Volume of Tubing
7.2
7.2
7.2
7.2
7.2
7.2
Voume of System
132.3
132.3
132.3
132.3
132.3
132.3
Mols of Gas Generated
0.00299
0.00325
0.003
3.397x10^-4
2.997x10^-4
3.297x10^-4
Theoretical Pressure
0.532
0.601
0.554
0.0628
0.0554
0.0609
Pressure Initial
0.9384
0.9366
0.9366
0.9366
0.9366
0.9366
Pressure Final
1.2388
1.2276
1.3102
1.009
1.006
0.9966
Change in Pressure
0.3004
0.291
0.3736
0.0724
0.0694
0.06
Percent Error
43.5
51.6
32.7
15.29
25.27
1.48

Calculations and Analysis

Balanced Equations
Mg(s) + 2HCl(aq) -> MgCl2 (aq) H2 (g)
Na2CO3(s) + 2 HCl(aq) -> 2NaCl(aq) + CO2(g) + H2O
CaCO3(s) + 2HCl(aq) -> CaCl2(aq) + CO2(g) + H2O

Preliminary Calculations

N=(0.5)(0.125L)/(0.08206 L*Atm/mol*K)(298 K) = 0.003 mol
0.003 is the same for the Gases. (H2 or O2)

-Amount of Solid needed to react w/ 1.0 M of HCl (Limiting Reactants)

CaCO3 (s) + 2 HCl (aq) -> CaCl2 (aq) + CO2 (g) + H2O (l)

Mg (s) + 2 HCl (aq) MgCl2 (aq) + H2 (g)

Minimum Amount of HCl Needed

*Add an extra 10 mL of HCl to make a minimum of 16 mL used for each reaction

-Experimental P (Pf - Pi)

Experimental Mg Average
(1.2589)-(.9372)=.3217

Experimental CaCo3 Average
(1.009)-(.9366)=.0724

Number of Mols Generated for Each Solid for all trials
CaCO3
Trial #1

Trial #2

Trial #3

Mg
Trial #1

Trial #2

Trial #3

Theoretical Pressure (Avg. Mols for Mg & CaCo3)

= .562 atm

= .0597 atm

Percent Error
Mg
Trial #1

Trial #2

Trial #3

CaCO3
Trial #1

15.29%

Trial #2

25.27%

Trial #3

1.48%

Discussion
Discuss your results and observations here. Keep in mind that this is the most important section of the report. Summary: An informative, detailed summary of your relevant results and observations. How did the amount of gas produced by the reaction compare to the amount that was predicted from stoichiometric and idea gas calculations? Goals: A discussion of how and whether the reasons and goals for this investigation were met. If they...