Flame Test Lab Report

The purpose of this lab is to observe how heat is released or absorbed with different chemicals.

Examine a piece of nichrome wire. On the data sheet, record the color and the luster of the metal. Use a forceps to hold the wire in the flame of your burner for about two minutes (recall where the hottest part of the flame is located). Describe the appearance of the wire while held in the hottest part of the flame. Allow the wire to cool and reexamine it. From your observations, determine if there was a physical or a chemical change. Give specific reasons for your conclusions. Save the nichrome wire for step #2.

Hypothesis: Reaction 3 will create the highest exothermic reaction in the test tube this is because the chemicals are highly flammable the means they are high in exothermic relations. If we use 4 grams of zinc powder the chemical retain with the copper sulphate solution will create the highest temperature We changed the

4. Why does the flame color change back to orange, after the metallic solution has been turned completely into a gas

This is done through a change in temperature. Over time, two objects that are in direct contact will

Allow the candle to burn for a few minutes noting any changes. 4. Blow out the candle and immediately place a lit match in the smoke just above the wick. Observe and record what happens. 5.

To perform the experiment, you need 2 ml of water, then contain 15 ml of 3m HCL, 6m HNO3, 6M NaOH, then 15 ml of unknown solution each one labeled on a test tube. A flame test will be conducted to determine ions. You will need a spot plate, Bunsen burner, flame-test wire, dropper bottles of 0.1 M NaCl, 0.1 M KCL, 0.1 M CaCl2. Obtain a spot plate. Place 5 to 8 drops of 0.1 M solutions of each of the following solutions into separate indentations: KCL, CaCl2, NaCl, unknown solution. To clean the flame-test wire dip the loop at the end

To improve the experiment, the methodology could be improved by having an efficient calorimeter to retain as much heat as possible, rather than just a tin can. Additionally, more trials for each of the experiments could be conducted to ensure correct and precise data is collected to determine more accurate conclusions.

Flame Lab Part 1. In the first part, a stick with strontium chloride on it was put into flames produced by a bunsen burner. This flame was red from the strontium chloride. The particles moved to an excited state and the color red was the result of the change of state.

2) A pair of safety goggles were worn according to the rules of the lab safety guidelines. 3) A candle was placed on top of a paper towel so the lab bench was protected against wax leaks. Then, the candle was lit carefully with a BBQ burner. 4) A timer was prepared to record the duration time of the flames. 5)

The wire loop was cleaned by dipping it in hydrochloric acid and rinsing it with deionized water. A Bunsen burner was lit, and the loop was put in the flame to see if it produced a color. If so, it was cleaned again. The wire loop was then dipped in the solution to be tested and put in the blue part of the

The phenol red was yellowish-orange at the top of the test tube, towards the bottom of the test tube the color turned into a deeper red. CO₂ (g) + CuO CH₄ + O₂ CO₂ + H₂O Zn + HCl Part C) When the HCl made contact with Zinc, a reaction happened immediately, gas was very rapidly produced. As the wooden splint was placed in the test tube containing gas, the fire went out and made a high pitched pop sound.

The wooden splint was placed in the flame and the flame colour was observed and recorded. 7. The used wooden splint was placed in the waste beaker. 8.

The random errors experienced in this experiment impacted the results gathered from experiment a lot less than the systematic errors. 1. Flame was not concentrated on the same point of the beaker. While conducting the experiment, there were small draughts through out the lab, which caused the movement and change of position of the heat energy of the flame.

In this project we examined three explanations that talk about (a) candle(s) in a jar and their investigation reasoning to why the labs they did were concluding in such a way. The first explanation resulted that the candle inside the jar took up all the oxygen molecules inside the flask which then lowers the pressure inside and the higher pressure outside the flask is what causes the water to rise up. The second explanation resulted in that the air pressure increases inside the jar because of the heat from the candle, which causes air to come out of the jar and once the candle cools down the pressure decreases and the pressure outside the jar increases which results in pushing the air in and making the water rise up. The third explanation resulted in oxygen inside the flask becoming carbon dioxide which then dissolves in water causing the air pressure to decrease under the glass and the higher pressure outside the flask pushed the water up the flask. I believe that explanation number three is right because the flame causes carbon dioxide to be created and that