Timer
Mass of Zn
Volume of HCl
Size of the stopper
Controlling Variables
size of test tube- we used the same test tube for most of the trials
syringe type- we used the same syringe for all the trials
timer- we used the same timer for all the trials
mass of zn- we kept the mass of zn constant 1.00g
size of the stopper- we used the same stopper
Procedure
- Grab a test tube rack, a test tube, a stopper that fits snuggly into the test tube and a syringe.
- Place the test tube into the test tube rack and attach the syringe to the test tube.
- Using an electric balance, obtain a sample of powdered Zn that weighs 1.00 g exactly.
- Pour the 1.00g sample of powdered Zn into the test tube.
- Grab two beakers. Fill one with HCl and the other with non-distilled water. BE SURE TO LABEL THE BEAKERS APPROPRIATELY!
- Using a 10ml graduated cylinder and pipette, measure out 10 ml of HCl.
- Pour the HCl into the test tube, quickly cork the test tube with the stopper, and pull slightly on the syringe’s end to make sure the hydrogen gas will flow through.
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Record the how long it takes for the marker on the syringe to reach, 1, 2, 3, 4, and 5 cm3.
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Repeat with HCl concentrations of 0.8 mol dm-3 and 06 mol dm-3.
- Repeat steps 3-9 a second time in order to obtain a second trial.
Data Collection and Processing
Raw Data Table
Hydrochloric acid, 1.0 mol dm-3
Hydrochloric acid, 0.8 mol dm-3
Hydrochloric acid, 0.6 mol dm-3
Observations
- Zn clumps together at bottom of test tube
- Bubbles are produced
- No longer powder
- Nothing happens for a while and then all of a sudden there’s like this outward burst of energy which results in small intervals btw the given volumes produced
Data Processing
Overview
I will first determine the average time it took for the different HCl concentration to react and produce the given volumes of hydrogen gas. Next I will calculate the standard deviation for each set of trials to determine the accuracy of the average. Finally, I will graph the average times using a scatter.
Sample Calculation
Average of different trials for time taken for 1cm3 of hydrogen gas to be produced with 1.0 mol dm-3 of HCl:
(118 + 123)/2 = 120.5s
Hydrochloric acid, 1 mol dm-3
Hydrochloric acid, 0.8 mol dm-3
Hydrochloric acid, 0.6 mol dm-3
Standard deviations of the averages were determined by using the following formula in a Microsoft Excel program:
Standard Deviation for different HCl acid concentrations
Average time vs. Volume of hydrogen gas produced
Conclusion and Evaluation
Conclusion:
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Hydrochloric acid, 1 mol dm-3 concentration, the highest concentration used in this experiment produced the given volumes of hydrogen gas the fastest out of all three HCl concentrations.
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Hydrochloric acid of 0.8 mol dm-3 concentration did produce 1 cm3 of hydrogen gas faster than hydrochloric acid of 0.6 mol dm-3 as predicted.
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Hydrochloric acid of 0.6 mol dm-3 concentration produced hydrogen gas faster than hydrogen gas of 0.8 mol dm-3.