Essay on Pre Lab Experiemnt 8

2. Summarize the following description of a chemical reaction in the form of a balanced chemical equation?

The objective of this experiment was to calculate the percentage of copper in three random pennies by applying

Mole of chlorine : 1.0217g - .221g - .3946 g = .4061 g of chlorine

The purpose of this lab was to make a substitutional alloy coating the penny in a gold color. The color of the penny depends on the Zinc and Sodium Hydroxide solution, and if heat was added or not. We took a copper penny and boiled it in a Zinc and Sodium Hydroxide solution. Then we took the penny out, rinsed it in water, and dried it off. Now the penny was silver. We then took the penny and waved it across a flame causing it to turn gold. Some errors that happened were getting Zinc in our water and over cooking the penny. These could be fixed by rinsing the Zinc off the penny in its solution before taking it out and not heating the penny for as long. A suggestion for improvement would be getting the flame at the lowest temperature possible.

3. Find the number of atoms of each of the substances involved in the reaction.

4. NaOH, sodium hydroxide is a strong base. It reacts with HCl and forms NaCl and H2O.

11. Write the balanced chemical reaction of zinc with HCl (same as problem 5). Is the product of

Write a balanced chemical equation for each reaction #1-8. Classify each reaction using the information provided in the

-If the copper metal is submerged in the silver nitrate solution then in reaction, a pure, solid (Ag) silver product is created with an excess of (Cu (NO3)2) copper (II) aqueous liquid because a single displacement reaction occurs where the balance equation is then

3) Repeat the drying process just to be sure that the copper is completely dry, and again determine the mass of the copper and the beaker.

Focus Question: Zn(OH)2 was the product when zinc and iodine were reacted without the presence of acetic acid in the water.

We began this experiment by obtaining and measuring the mass of a 20 x 150 mm test tube and a 22 x 175 mm test tube with boiling stones. We then weighed out 2 grams of zinc and iodine. First, we added the zinc to the 20 x 150 mm and weighed it out. Then we added the iodine to the 20 x 150 mm and weighed it out. This gave us the amount of each element we were working with before the reaction. Next, we made weak acidified water by adding 18 drops of acetic acid to 25 mL of distilled water in a 50 mL beaker. Then we added 5 mL of acidic solution to the 20 x 150 mm test tube. After the solution is added we swirled the test tube until the liquid became colorless. Once colorless, we poured it into the 22 x 175 mm test tube. We repeated mixing the acid with the zinc and iodine two more times. Then we repeated it 3 more times but poured the solution down the drain. Furthermore, we used a bunsen burner to softly dry off the zinc in the 20 x 150 mm test tube. Once, completely dry we let the test tube

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

In the lab, Molar Volume of an Ideal Gas, different amounts (in mL) of 6 M HCl were added into a beaker with various amounts (g) of zinc (Zn). In the first test, 10 mL of HCl were added into a beaker with 0.25 g of Zn. The moles of zinc reacted were 0.00382, and this is the same number for the moles of hydrogen produced. In the second test, 10 mL of HCl was added as well as 0.5 g of Zn. The total moles of zinc reacted were 0.00765 and 0.00765 moles of hydrogen were produced. In this reaction zinc was the limiting reactant. The percent error in the reaction was 0.083%.

Then in phase three which was titled Temperature and that was steps 15-18, clean zinc was placed in three different test tubes containing 5ml of 6M HCL, each of which was a different temperature. Test tube one was placed in boiling water, Test tube 2 was at room temperature and test tube three was placed in an ice bath. When the zinc was placed in test tube 1 it reacted quickly and