8. Balanced chemical equation for the formation of zinc chloride from zinc and HCl First, we set up the equation xZn(s) + yHCl(aq) → ZnxCly (s) + y/2H2(g) . We knew the empirical formula for zinc chloride is ZnCl8. Based on the law of conservation of matter, we got the balanced equation:
Balanced equation: Zn(s) + 8 HCl(aq) → ZnCl8 (s) + 4 H2 (g)
9. Percentage Error Calculation: Experimental values: (1.8+4.34)/2= 3.07g (average mass) Accepted values: 2.67g ZnCl8 0.5g Zn x 1mol Zn/65.4g Zn x 1/1 x 349.4g ZnCl8/ 1 ZnCl8 mol = 2.67g ZnCl8 l 3.07g-2.67gl / 2.67 x 100 = 14 %
B Copper Sulfide
Trial 1 Trial 2 Trial 3
1.Mass of crucible, cover and copper 22.82g 21.04g 22.87g
2.Mass of crucible and cover 20.91g 20.61g 21.49g
3.Mass of
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And the mixture turned black after heated it with strong flame for 5 minutes. The mass of copper was found by subtracting the mass of crucible and cover from the mass of the crucible, cover, and copper. Also, the mass of copper sulfide was calculated by subtracting the mass of crucible and cover from the mass of crucible, cover, and copper sulfide. Then the mass of copper sulfide was subtracted by the copper to get the mass of sulfur.
7. Empirical Formula for copper sulfide:Cu2S
In order to determine the empirical formulas, the mass in grams is converted to moles.
Average mass of copper: 1.24g Cu
Average mass of sulfur: 0.28g S
1.24g Cu X 1 mol Cu/ 63.55g Cu = 0.0195mol Cu
0.28g S X 1 mol S/ 32.07g S = 0.0087mol S
Then, to find the smallest whole number ratio, we divided each number of moles by the smallest number. The ratio is 2Cu:1S, so the empirical formula is Cu2S
0.0195mol Cu / 0.0087mol S= 2
0.0087mol S / 0.0087mol S = 1 8. Balanced chemical equation for the formation of copper sulfide from copper and sulfur.
First, we set up the equation xCu(s) + yS(s)→ CuxSy (s) . We knew the empirical formula for copper sulfide is Cu2S. Based on the law of conservation of matter, we got the balanced equation:
2Cu + S = Cu2S
9.Percentage Error
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Can you determine the molecular formula of a substance from its percent composition? A: Yes.
2. Given that zinc chloride has a formula weight of 136.28 amu, what is its formula? A: ZnCl2
3. Can you determine the atomic weights of zinc or copper by the methods used in this experiment? How? What additional information is necessary in order to do this? A: Yes, we need molar mass of sulfur, hydrogen, and chlorine. Then set the molar mass of copper and zinc to x and y. And use the mole ratio, which is 1:1 for two reactions to solve the unknown.
4. How many grams of zinc chloride could be formed from the reaction of 3.57g of zinc with excess HCl? A: 3.75g x 1mol/ 65.39g x 1 mol/ 1mol x 136.4g / 1 mol = 7.45g.
5. Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. (a) Write a balanced equation for this reaction. (b) How many grams of aluminum hydroxide can be obtained from 10.5g of aluminum sulfide? A: (a): Al2S3 + 6 H2O → 2 Al (OH)3 +
An error that could have been present during the lab includes not letting the zinc react completely with the chloride ions by removing the penny too early from the solution. For instance, the percent error of this lab was 45.6%, which was determined by the subtraction of the theoretical percent of Cu 2.5% and the experimental percent of Cu 3.64% and dividing by the theoretical percent of Cu 2.5%. This experiment showed how reactants react with one another in a solution to drive a chemical reaction and the products that result from the
Discussion 1. Zn0 (s)+ Cu2+S6+O42-(aq) →Cu0(s) + Zn2+S6+O42-(aq) Zn0(s) → Zn2+(aq) + 2e- Cu2+(aq) + 2e- → Cu0(s) Zn0(s) + Cu2+(aq) → Zn2+(aq) + Cu0(s) Oxidant (oxidizing agent) is the element which reduces in experiment.
Then the mass of the copper metal and the percentage of Cu were obtained and compared throughout different groups and a mean and standard deviation was calculated for the
After copper ions were filtered, approximately 15mL of .5 M was added to the filtrate, which made the mixture acidic. Then, 20 mL was added into the filtrate to raise the pH of the mixture.
In order to begin this experiment, first one must find the balanced chemical equation for the reaction which occurs between the aluminum and copper (II) chloride. This balanced equation being 2Al(s)+3CuCl2 (aq)3Cu(s)+2AlCl3 (aq). After finding this equation, one must use the process of stoichiometry in order to find how many grams of aluminum are needed in order to produce 0.15 grams of copper. In this experiment, the purpose was to produce between 0.1 and 0.2 grams of copper, so one should attempt to produce 0.15 grams of copper seeing as it is the average of those two numbers. The first step in the stoichiometric process which one has to complete is finding how many grams of copper are in one mole of copper.
After I rinsed the copper I transferred it to a watch glass that had been baked for 20 minutes so it would not contain any liquid so as to not counteract the experiment. After I put the copper on this watch glass I baked the copper in the oven for 20 minutes so there would be no liquid left in that to mess up the mass. After 20 minutes I removed the watch glass with the copper in it and weighed itm making sure to weigh the watch glass
Copper is a chemical element with the symbol Cu and atomic number twenty-nine. It is also a solid at room temperature. Copper was most likely the first element ever manipulated by humans. In fact, humans discovered copper during the Paleolithic era. Copper was also very important during the copper and bronze age.
To better understand this law, Cu(s) was transformed with different reactions only to return back to Cu s). The initial and final mass of Cu(s) was recorded to give the percent recovery of copper product at
Purpose: The purpose of this lab is to titrate an unknown solid acid (KH2PO4) with a standardized sodium hydroxide solution. After recording and plotting the data, the acid’s equivalence point will be recorded once the color changes. Using the equivalence point, the halfway point will be calculated, which is used to determine the acid’s equilibrium constant. The acid’s calculated equilibrium constant will be compared with the acid’s established pKa value.
Using the equation m = ΔTf/Kf , the molality of the unknown solution was found. Then, moles of unknown were calculated, which was used to calculate the average molar mass of unknown. Theory: After the experiment was completed, the data
The zinc will form a new compound with the sulfate, and the copper will stay as a metal. Balanced Chemical
The percent recovery of the copper was calculated using the equation, percent recovery = (the mass of the copper recovered after all the chemical reactions/the initial mass of the copper) x 100. The amount of copper that was recovered was 0.32 grams and the initial mass of the copper was 0.46 grams. Using the equation, (0.32 grams/0.46 grams) x 100 equaled 69.56%. The amount of copper recovered was slightly over two-thirds of the initial amount.
Using the Law of Definite Proportions, the mass of this product was used to determine the number of moles of copper and chlorine in the sample, which led to being able to determine the
Verna Wang Hannah Palmer CHEM 101-069 Lab 11-19-16 Stoichiometry and Limiting Reagents Lab Report Purpose: We are using the reaction of sodium hydroxide and calcium chloride to illustrate stoichiometry by demonstrating proportions needed to cause a reaction to take place. Background: Just like a recipe would call for a specific amount of one ingredient to a specific amount of another, stoichiometry is the same exact method for calculating moles in a chemical reaction. Sometimes, we may not have enough of or too much of one ingredient , which would be defined as limiting and excess reagent, respectively.
After the reaction is finished, the percentage composition of each element in the product can be found and used to calculate the empirical formula, which is the lowest whole number ratio