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In Millikan's Oil Drop Experiment, the charge of the electron was determined to be approximately x10-17 C. This result yielded a significant error because the accepted value for the charge of the electron is 1.6 x 10-19 C. Millikan's conclusion about the size of the electron's charge was based on the observation that his experimental results were explainable as multiples of 1.6 x 10-19 C. For this experiment, the calculated value for the multiple was 1.30 x 10-17 C. The large error in the result may be attributed to instrument wear, inaccurate observations, incorrect voltage applied to the plates, or plate wear.
Millikan's Oil Drop Experiment aimed to determine the charge of the electron by observing the motion of tiny oil droplets in an electric field.
The experiment provided valuable insights into the atomic nature of electricity, demonstrating the participation of atoms in conducting electricity. Millikan's conclusions were drawn from repeated experiments, where he noticed that the results were consistent with multiples of the accepted electron charge.
The following materials were used in the experiment:
The experimental setup involved suspending tiny oil droplets in an observation chamber.
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A voltage was applied across the plates in the observation chamber, creating an electric field. By adjusting the voltage, Millikan was able to observe the motion of the oil droplets and calculate their charge-to-mass ratio. From these observations, he determined the charge of the electron.
The experiment's data analysis involved tracking the motion of oil droplets in the electric field.
By measuring the droplets' velocities and applying the known forces of gravity and buoyancy, Millikan calculated the charge-to-mass ratio for each droplet. The charge-to-mass ratio was determined using the following formula:
Charge-to-Mass Ratio (q/m) = (mg) / (E * v)
Where:
By collecting data from multiple droplets and calculating their charge-to-mass ratios, Millikan determined the charge of the electron. The results were analyzed and compared to the accepted value of the electron charge to assess the accuracy of the experiment.
The experimental results indicated that the charge of the electron, as determined by Millikan, was approximately x10-17 C. However, this value exhibited a significant error when compared to the accepted value of 1.6 x 10-19 C. The discrepancy in the results may be attributed to various factors:
Despite the large error in the calculated charge, Millikan's conclusions were based on the observation that the results were consistent with multiples of the accepted electron charge.
The Millikan Oil Drop Experiment provided important insights into the atomic nature of electricity. It demonstrated that electricity involves the exchange of electrons, and atoms play a crucial role in conducting electricity. The experiment's results, while exhibiting a significant error compared to the accepted value, were consistent with the idea that the electron charge is quantized in multiples of 1.6 x 10-19 C.
In conclusion, Millikan's Oil Drop Experiment aimed to determine the charge of the electron. While the calculated value of the electron charge exhibited a significant error when compared to the accepted value, the experiment's methodology and setup were consistent with those used by Robert Millikan. The experiment provided valuable insights into the atomic nature of electricity and contributed to our understanding of the role of atoms in conducting electrical charge.
Further studies in experimental physics can help refine the accuracy of experiments like the Millikan Oil Drop Experiment. Investigating potential sources of error and improving the experimental setup can contribute to more precise results. Additionally, exploring the quantization of electric charge in other contexts can expand our understanding of fundamental physics principles.
Millikan's Oil Drop Experiment Report. (2016, Oct 11). Retrieved from https://studymoose.com/document/millikan-oil-drop-experiment
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