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Rock Street, San Francisco

Brinkley Morse
Carrier A
11/17/17

Chemical Equation: 2Mg + O2? 2MgO
In this reaction, magnesium metal was burned in oxygen gas to produce magnesium oxide. The original magnesium metal was malleable and silver, and the oxygen gas was invisible and odorless. The product, MgO, was white and powdery. Once place over the bunsen burner, the magnesium strip began to glow red and then a bright white. Once could guess that the product of the reaction would be MgO, since the reaction is simple synthesis. Also, the substance generated by the reaction closely resembled Magnesium oxide, so, along with the prediction in the chemical equation, it can be assumed that the product is in fact MgO.

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Chemical Equation: CuCO3 + heat ? CuO + CO2
In this reaction, copper II carbonate decomposes to produce CO2 and Copper Oxide. The original CuCO3 was a green powder. CO2 and CuO were products of the reaction. CO2 was an odorless and invisible gas and the produced CuO was a black powder. During the reaction, the copper II carbonate changed color from green to black as gradually turned it to copper oxide. This was a decomposition reaction. The burning the splint going out would have indicated the presence of CO2, however, it did not.

Chemical Equation: CuSO4+Mn? Cu + MnSO4
In this reaction, copper II sulfate and manganese reacted to produce copper metal and manganese sulfate solution. The CuSO4 was a clear, blue liquid and the manganese was a brownish metal. After the reaction, the CuSO4 lost its color, which signified that copper II ions left the solution. Small reddish-brown chunks were also observed. These chunks were likely copper metal, considering natural copper has a similar color pattern as the pieces observed in the solution. This was a single replacement reaction.
Chemical Equation: 2HCl + Mg ? H2 + MgCl2

In this reaction, hydrochloric acid reacted with magnesium metal to produce hydrogen gas and MgCl2. Hydrochloric acid was a clear, colorless liquid and the magnesium metal was a sliver strip. During the reaction, lots of bubbling occurred, which shows that a gas was produced. A burning splint was inserted into the tube and a loud pop was heard, which proves that hydrogen gas was the gas produced. The other product, magnesium chloride, was likely dissolved in the solution since no precipitate was produced. This was a single replacement reaction.
Chemical Equation: Na2CO3 + 2HCl? H2O +CO2 + 2NaCl

In this reaction, sodium carbonate reacted with hydrochloric acid to produce water, carbon dioxide, and table salt. Hydrochloric acid was a clear, colorless liquid and so was sodium carbonate. During the reaction, lots of bubbling was observed, which shows the production of a gas, which is likely CO2. The gas could have been proven to be CO2 if a burning splint were placed in the test tube and it went out, but such a test was never conducted. Sodium chloride was also produced, but it was dissolved in water so no physical evidence was present to prove ist existence. This was a double replacement reaction.
Chemical Equation: CaO + H2O? Ca(OH)2

In this reaction, calcium oxide reacted with water to produce calcium hydroxide. Calcium oxide was white powder and water was a clear, colorless liquid. The product of this reaction was calcium hydroxide, which was a white, opaque liquid. pH paper was placed in the test tube and turned from a beige color to a dark blue, indicating that the product was a base, which calcium hydroxide is. This was a synthesis reaction.
Chemical Equation: H2O2 ? (MnO2) ? H2O + 2O2

In this reaction, hydrogen peroxide was in the presence of MnO2 and decomposed into water and oxygen gas. The H2O2 was a clear colorless liquid and the magnesium oxide was a black powder. During the reaction, a great deal of bubbling was observed, which indicates that a gas was produced. A glowing splint was inserted into the test tube and reignited, which proves that the gas in question was oxygen. After the bubbling, the black powder at the bottom of the test tube seemed unchanged, which suggests that it was a catalyst in the reaction rather than a reactant. The other product was water, which was a clear colorless liquid. This was a decomposition reaction.
Chemical Equation: 2H2O + Ca? Ca(OH)2 + H2

In this reaction, calcium powder was mixed with distilled water to produce Calcium Hydroxide and hydrogen gas. Distilled water is a clear, odorless liquid and calcium is a soft, malleable metal. In this instance, calcium powder was used instead of solid calcium metal. The products of this reaction where hydrogen gas and calcium hydroxide. Hydrogen is a clear, odorless and highly combustible gas and Calcium Hydroxide is an extremely basic white, powdery substance. During the reaction, there was a great deal of bubbling, which shows the production of a gas (namely hydrogen). A burning splint was also inserted into the test tube, and a loud pop was heard afterwards, further proving the presence of hydrogen gas. After the pop, a white, slimy substance could be seen accumulating at the bottom of the test tube. This substance was calcium hydroxide. After the pop, a ph stip was used on the slime and said strip turned dark blue, indicating the presence of a base and further supporting that the slime was calcium hydroxide. This was a single replacement reaction.
Chemical Equation: Pb(No3)2 + 2KI? 2KNO3 + PbI2

In this reaction, lead nitrate and potassium iodide reacted to produce potassium nitrate and lead iodide. Lead Nitrate and potassium iodide were both clear, colorless liquids. KNO3 and PbI2 were produced from this reaction. During the reaction, the clear liquid turned a bright yellow. This likely happened because of the formation of PbI2, which is naturally a yellow powder. KNO3 also formed during this reaction. Considering that KNO3 is a clear salt, it likely dissolved in the solution. No tests were performed to verify its production, but if the liquid were evaporated, one could see solid KNO3 accumulate at the bottom of the well. This was a double replacement reaction.
Chemical Equation: Na2CO3 + Ni(NO3)2? 2NaNO3 + NiCO3
In this reaction, sodium carbonate reacted with nickel II nitrate to produce sodium nitrate and nickel carbonate. Na2CO3 and Ni(NO3)2 are both naturally solids, however they were both dissolve in water for the purpose of this experiment. The Ni(NO3)2 solution was slightly green. The products of this reaction were NaNO3 and NiCO3. NaNO3 is a white solid that is solvent in water and NiCO3 is a slimy, green compound. There was no obvious presence of NaNO3 since it dissolved in the solution, however if the solution were evaporated it would be possible to see solid NaNO3 crystals. The presence of NiCO3 was supported by the solution turning bright green as soon as the reaction occurred. Considering NiCO3 is naturally very green, the color change in the solution could easily be explained by said compound’s presence. This was a double replacement reaction.
Chemical Equation: 2AgNO3 + K2Cr2O7? Ag2Cr2O7 + 2KNO3
In this reaction, AgNO3 reacted with K2Cr2O7 to produce Ag2Cr2O7 and 2KNO3. AgNO3 and KNO3 are naturally solids, however they were both dissolve in water for this lab. Their solutions were both clear, colorless liquids. KNO3 and Ag2Cr2O7 were the products of this reaction. Considering that KNO3 is a clear salt, it likely dissolved in the solution. No tests were performed to verify its production, but if the liquid were evaporated, one could see solid KNO3 accumulate at the bottom of the well. Ag2CRO7 is a dark red, powdery solid. Its presence is supported by the solution turning a deep red once the chemical reaction began. Considering Ag2CRO7 is naturally crimson, the color change in the solution could easily be explained by said compound’s presence. This was a double replacement reaction.

Chemical Equation: C2H6O + 3O2 ? 2CO2 + 3H2O
In this reaction, ethyl alcohol combusted in oxygen to form CO2 and water. Ethyl alcohol is a clear, colorless and highly flammable liquid and oxygen is an odorless, invisible gas. The products of this reaction are the same as any combustion reaction, CO2 and H2O. CO2 is an invisible, odorless gas and water is a clear, colorless liquid. During the experiment, the ethyl alcohol was ignited. After the fire burnt out, liquid was left on the bottom of the jug. This liquid was water, considering all combustion reactions produce water. No test was performed to see if CO2 was produced, however, if a burning splint were placed in the jug and said splint went out, the presence of CO2 would be confirmed.

Double Replacement: 5, 9 , 10, 11

Single replacement: 3, 4, 8

Synthesis: 1, 6

Decomposition: 2, 7

Combustion: 12

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