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As pressure increases, volume decreases. As volume increases, pressure decreases.
Figure 2
The slope of this graph exemplifies a direct proportional relationship between pressure and the inverse volume. Figure 3
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Conclusion:
From this experiment, the relationship between pressure and volume is explored and analyzed. As volume increases, pressure decreases. As volume decreases, pressure increases. Thus, the pressure and volume of air (which is a mixture of several gaseous components such as nitrogen, oxygen, argon, and carbon dioxide) at a constant temperature (in this case, room temperature of 21.0 ± 1.0˚C.) have an inverse relationship (as shown in Figure 4 which exemplifies an exponential decay). This is also known as Boyle’s Law, which can be dated back to 1662. Also, from Avogadro’s Law, we can conclude that the pressure of a gas depends on both volume and temperature, but not composition of the gas or whether the gases are all the same or …show more content…
This reveals that pressure is proportional to the inverse of volume. The reason that pressure and volume are inversely related is because a gas is made up of loosely packed molecules moving in a random motion. When a gas is compressed in a container, the molecules are pushed closer, which results in a smaller volume that air occupies. The molecules now are forced to bounce in a closer proximity, which inevitably exerts more pressure. During my experiment, when I pressed the syringe down to a volume of 55 mL ± 0.5, the pressure gauge read approximately 90.5 mmHg (± 10.0) or (12.1 kPa ± 2.0). Then, when I pressed the syringe down even further to 45 mL ± 0.5, the pressure increased to 100.1 mmHg (± 10.0) (or 13.3 kPa ± 2.0). Theoretically, using the equationP1 V1=P2 V2, I calculated P2 to be 99.6 mmHg ± 10.0%, resulting in a tiny percent error of 0.50%. Even for all of the other trials, the percent error of all my experimental values didn’t exceed within a ± 3.0% of the theoretical values. Thus, my data is reliable and does not refute my hypothesis in that pressure and volume are inverse relationships of each …show more content…
However this equation is accurate enough for use in practical labs and applications. Thus, the data from this experiment is not exact, but relatively precise and accurate. Since the summary of percent uncertainty was greater than the overall percent error itself, this reveals that most of the errors occurred in the equipment itself (limitations of the equipment). Thus, my data is reliable because the percent error is not higher than my percent uncertainty which would indicate a mistake in the experimenter. However, there are several sources of errors which may have skewed the data. For example, air currents may have altered the volume and pressure of the air when we were compressing the syringe. Furthermore, again, there could have been a design flaw in the equipment of this experiment (such as a hole in the syringe, or broken pressure gauge). Ways to improve this lab is to take more trials with a greater and longer syringe. Furthermore, we could use different types of gases and see the effects of each on pressure and
Figure 2
The slope of this graph exemplifies a direct proportional relationship between pressure and the inverse volume. Figure 3
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Conclusion:
From this experiment, the relationship between pressure and volume is explored and analyzed. As volume increases, pressure decreases. As volume decreases, pressure increases. Thus, the pressure and volume of air (which is a mixture of several gaseous components such as nitrogen, oxygen, argon, and carbon dioxide) at a constant temperature (in this case, room temperature of 21.0 ± 1.0˚C.) have an inverse relationship (as shown in Figure 4 which exemplifies an exponential decay). This is also known as Boyle’s Law, which can be dated back to 1662. Also, from Avogadro’s Law, we can conclude that the pressure of a gas depends on both volume and temperature, but not composition of the gas or whether the gases are all the same or …show more content…
This reveals that pressure is proportional to the inverse of volume. The reason that pressure and volume are inversely related is because a gas is made up of loosely packed molecules moving in a random motion. When a gas is compressed in a container, the molecules are pushed closer, which results in a smaller volume that air occupies. The molecules now are forced to bounce in a closer proximity, which inevitably exerts more pressure. During my experiment, when I pressed the syringe down to a volume of 55 mL ± 0.5, the pressure gauge read approximately 90.5 mmHg (± 10.0) or (12.1 kPa ± 2.0). Then, when I pressed the syringe down even further to 45 mL ± 0.5, the pressure increased to 100.1 mmHg (± 10.0) (or 13.3 kPa ± 2.0). Theoretically, using the equationP1 V1=P2 V2, I calculated P2 to be 99.6 mmHg ± 10.0%, resulting in a tiny percent error of 0.50%. Even for all of the other trials, the percent error of all my experimental values didn’t exceed within a ± 3.0% of the theoretical values. Thus, my data is reliable and does not refute my hypothesis in that pressure and volume are inverse relationships of each …show more content…
However this equation is accurate enough for use in practical labs and applications. Thus, the data from this experiment is not exact, but relatively precise and accurate. Since the summary of percent uncertainty was greater than the overall percent error itself, this reveals that most of the errors occurred in the equipment itself (limitations of the equipment). Thus, my data is reliable because the percent error is not higher than my percent uncertainty which would indicate a mistake in the experimenter. However, there are several sources of errors which may have skewed the data. For example, air currents may have altered the volume and pressure of the air when we were compressing the syringe. Furthermore, again, there could have been a design flaw in the equipment of this experiment (such as a hole in the syringe, or broken pressure gauge). Ways to improve this lab is to take more trials with a greater and longer syringe. Furthermore, we could use different types of gases and see the effects of each on pressure and