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04.05 Chemical Reactions: Combustion

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zoey ramsay

on 26 September 2013

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Transcript of 04.05 Chemical Reactions: Combustion

04.05 Chemical Reactions: Combustion
Zoey Ramsay :)
Data and observations
Detail 1
Write a balanced equation for each reaction observed in this lab. (10 points)

Detail 2
If you were to measure the mass of magnesium and hydrochloric acid before combining them in the test tube, how would that mass compare to the mass of reactants left in the test tube after the reaction? Explain your answer and how it corresponds to the law of conservation of mass. (5 points
Detail 3
One of the reactions you conducted can actually be categorized as TWO different types of reactions. Which reaction is this, and what are the two types of reactions? (5 points)
Iron and copper (II) sulfate solution
Fill a small test tube halfway with copper (II) sulfate solution. Add one or two scoops of iron metal shavings to the solution and observe the reaction.

Observation: The iron shavings are initially dark gray, and the copper (II) sulfate solution is a transparent blue solution. When they mix together, the blue color of the solution fades slightly while the iron shavings change to a dark reddish brown color in the test tube.
Lead (II) nitrate and potassium iodide solutions
Pour about 2.0 mL of lead (II) nitrate into the test tube. Add five to ten drops of potassium iodide solution to the test tube and record your observations of the reaction.

It would be the same mass because according to the law of conservation of mass, energy cannot be created or destroyed; only changed
it would be the hydrochloric acid and the magnesium because it bubbled, but still stayed in its form and didn’t change.
Iron and copper
lead and nitrate
magnesiam and metal
Electoyls of water
burning magnesium
copper will melt
lead will melt
metal will melt
water will bubble
magnesium will melt
it bubbled
it mixed together but sunk
didnt melt
did not melt
Observation: Both solutions are colorless and transparent, but when they combine an opaque yellow solid is formed.
Magnesium metal and hydrochloric acid solution
Pour hydrochloric acid solution into a test tube and then add a small strip of magnesium metal ribbon to the same test tube.

Safety Warning: Hydrochloric acid is corrosive; if you spill any on yourself flush it immediately with water and notify your teacher.

Observation: When the magnesium metal is added to the hydrochloric acid solution, a lot of bubbling occurs on the surface of the metal.

Electrolysis of water
Use a U-tube with electrodes at each end, connected to a battery. When the battery is turned on, observe the results at each electrode.

Observation: When the battery is turned on, bubbling occurs at each electrode. There seem to be more bubbles produced at the electrode labeled “H2” than at the electrode labeled “O2.”

Burning magnesium
Turn on a Bunsen burner, and use forceps or a spatula to hold a small piece of magnesium metal ribbon in the flame.
acid base
double displacement
2Fe + 3CuSO4 --> Fe2(SO4)3 + 3Cu
Pb(NO3)2 + 2KI --> PbI2 + 2KNO3
Mg + 2HCl --> MgCl2 + H2
electricity doesn't 'shock' water. shock only comes from the impurities found in water that is not distilled. anyway.....2H2O --> 2H2 + O2
2Mg + O2 --> 2MgO
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