How Voltage Is Affected Within A Cell

To determine which ions are present in the two unknown solutions. This will be accomplished by mixing three known solutions with three testing solutions. You will use this information to determine which ions are present in the unknown solutions.

The experiment procedure is first, get your materials, shells, water, vinegar, measuring spoon, a cup, and a beaker. Next,

this experiment had a similar scenario to part A except the metals were switched and replaced with

Obtain a 50 mL beaker for the experiment. In the first part of the experiment, you dissolve the zinc core of a penny and leave the copper covering intact by putting four notches in

In Part 1 of the lab, a solar cell was created and tested for its capability to conduct electricity. After researching the processes that contribute to the conductive property, it was found that the oxidized substance is the dye, as it donates an excited electron to the titanium oxide. Consequently, titanium oxide is reduced before it donates an electron to the cathode. The electrolyte solution was found to replenish the dye with electrons so it could continue to act as a reducing agent.

Part 1: Obtain some 0.200M Fe(NO3)3 solution and some 0.00020M KSCN solution. Starting from the first solution, pour and mix 8.0mL of Fe(NO3)3 solution and 2.0mL of KSCN solution into a test tube, where as the second solution has 7.0mL of Fe(NO3)3 solution and 3.0mL of KSCN solution. Continue this process until 5 test tubes have been filled. Pour

In this lab we will be heating up substances and use them to galvanize pennies. When you heat up the zinc, and then coat the penny in it, it then galvanizes the penny. Meaning, it helps protect the penny from oxygen and water. Afterwards, you will need to record data such as the mass of the penny. This helps keep track of what physical traits are being changed during this experiment. On part B of this experiment, you will be heating up the now galvanized pennies in order to see what reaction you get. The reaction you should receive from heating up the now zinc-covered pennies is that the pennies will change color.

In Lab 8, the time constant of resistance-capacitance was measured in order to determine the charge of a capacitor. This experiment was conducted by setting building a circuit that connects the voltmeter across the resistor. The voltmeter was then connected across the capacitor. The above procedure was conducted several times using different voltages. Afterwards, the results were calculated and tabulated. The data obtained from the lab were the theoretical Tau for 5V, 4V and 3V. In this experiment, the calculated voltage was also determined. The theoretical and the calculated values were then compared and evaluated by determining their percentage errors. For example, in the 5V, the theoretical value was 1.23V; calculated value was 1.434 with a percentage error of 16.6 %( for voltmeter across capacitor).

Then I attached the black clip to the coin and the red clip to the copper strip. I then placed each item in the copper sulfate solution and attached the opposite end of the black clip to the negative side and the red clip to the positive side of the battery. Then I waited ten minutes to observe the effects on the items. I then re-cleaned both items and followed the above steps, except the clips. I placed the red clip on the negative side and the black clip on the positive side of the battery. I performed this experiment with the coin and copper strip first and then re-performed the same experiment with the key and copper

The same directions in Part A were repeated, using different metals and solutions. Fe Cu Zn

The main objective of this experiment is to carry out qualitative analysis to identify metal cations in unknown solution 1.

Next assemble the digital multimeter or voltmeter so the black lead is in the hole labeled COM. Make sure the voltage is set to 0.00. Use the test lead attached to the penny (red) and place it into the volts (VΩmA) hole. After setting up the fruit and digital multimeter or voltmeter, use the timer and set it for 10 seconds and allow the voltage to settle. After ten seconds record the voltage

The prepared zinc powder could easily be removed from the cathode surface and was washed in distilled water for several times until all possible existing alkaline solution was removed from the powder particles. This was proved by addition of few droplets of phenolphthalein to the ablution water. After that, the powder was treated with an alcohol-acetone mixture (ethanol-acetone = 1:1) to remove water, then dried for 2 h in 100 °C, weighed, and stored in a polyethylene plastic bag to avoid further oxidation. A different weight of Zn powder was obtained in each experiment, the current efficiency (CE) was calculated using Eqs. (1) and (2) as follows:

Let the set-up stand for 15 minutes until the temperature stabilizes. 4. Pour about 5 ml of 0.1 M KNO3 into the center well. Pour about 5 ml of 0.50 M ZnSO4 into well #1 and about 5 ml of 0.50 M CuSO4 into well #2. 5. With clean tweezers, take a s trip of filter paper and dip one end into the central well (where immersion in the KNO3 solution will hold one end); dip the other end into well #1. Repeat this procedure with another strip of filter paper, dipping the other end into well #2. This creates the salt bridge for your galvanic cell. 6. With clean tweezers take a zinc metal strip and sand it (on a piece of paper so as not to scratch the table top) to remove any oxide coating. Bend 2 cm of one end of the ªS trip and immerse it in the ZnSO4 solution (well #1). The rest of the metal strip (3cm) extends out to the edge of the cell and should be bent over the rim. Repeat the same procedure with the copper metal strip and place it in well #2. Later the electrical leads (alligator clips ) from the interface will be attached to the metal strips. 7. Fasten your temperature probe to the ring stand with a clamp and adjust the temperature probe such that its tip can be immersed in the central well (KNO3 solution) of the cell. It is assumed that the temperature of the ZnSO4 solution and CuSO4 solution will be very close to the temperature of the KNO3 solution throughout the experiment. 8. Start the computer program to

At the end of the experiment when the lid was removed, it was found out that the blue colour of the copper (II) sulphate solution has faded away. It was turned to pale grey and there were some precipitates present. It was the zinc powder that was in excess to ensure that the copper (II) sulphate solution could react fully with the zinc powder.