Balanced Chemical Equation: Cu(s) + 4HNO3(aq) —> Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O (l) Reaction 2: when sodium hydroxide (NaOH) is added to copper (II) nitrate (Cu(NO3)2), a double displacement reaction will occur. Copper and sodium will displace each other to create copper (II) hydroxide and sodium nitrate. Balanced Chemical Equation: Cu(NO3)2 (aq) + 2NaOH (aq) —> CuOH2 (s) + 2NaNO3 (aq) Reaction 3: When copper (II) hydroxide is heated, a decomposition reaction will occur. The reaction will decompose forming two compounds, Copper (II) oxide, and water. Balanced Chemical Equation: Cu(OH)2 (s) + Heat —> CuO (s)
In this experiment, a balanced chemical equation will be provided for decomposition reactions. A redox reaction is a reaction where one reactant is reduced due to a gain of electrons, and the other is oxidized due to a loss of electrons. The reactant that loses an electron is called the reducing agent, whereas the reactant that gains an electron is called the oxidizing agent. In this experiment, the balanced chemical equation, and the two half equations for the redox reactions will be provided, and the oxidizing and reducing agents will be
The items that were massed were the evaporating dish, watch glass, and NaCO3. The materials were massed once before and once after being heated in the drying oven. The mass of the evaporating Dish before was 46.57 g; while after being heating was 60.15 g. The mass of the watch glass before was 57.97 g and after was 48.75g. There were two masses taken for the substance NaHCO3- one with the evaporating dish and one without, subtracted out after the lab was concluded. The mass of the substance with the dish was 48.79 g before and 62.33 g after; meanwhile, the mass of the substance without the dish was 2.22 g before and 2.18 g after. The mass of the NaHCO3 had changed after the reaction occurred along with after it was placed on the hot plate and being in the drying oven.
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.
Everything can change from one substance to another, but the creation and the end of some things never happen .On a beautiful day on the fourth of December in 2015, the class of SNC1D5 started a lab on different kinds of molecules. The reason why we did this lab was to investigate the chemical and physical changes between different substances. Substances can change from one substance to another that have alternate physical and chemical properties by chemical reactions or with reactants or with heat. A physical change mixes up molecules but doesn’t hurt their inner structure. An example of physical change is ice turning into water due to heat because it didn’t change the substance’s material. A chemical change occurs when there’s a new arrangement
Introduction : The percent composition of a compound can be found by determining the mass of each element within that compound, and with this information, the empirical formula can be determined. The lab consisted of obtaining a magnesium ribbon and having it undergo chemical reactions to create solid magnesium oxide with the aim being identifying the percent composition and empirical formula of the compound. Background Information : To determine magnesium oxide’s percent composition and empirical formula, the masses of magnesium and oxygen separately must be found and then divided by the total mass and multiplied by 100 to find the percent makeup of each element within the compound. However, to obtain magnesium oxide, it had been synthesized from magnesium and various chemical reactions with only the initial mass of magnesium and the final compound’s mass being known.
Experiment 2 Report Scaffold (Substitution Reactions, Purification, and Identification) Purpose/Introduction 1. A Sn2 reaction was conducted; this involved benzyl bromide, sodium hydroxide, an unknown compound and ethanol through reflux technique, mel-temp recordings, recrystallization, and analysis of TLC plates. 2. There was one unknown compound in the reaction that was later discovered after a series of techniques described above.
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 0.5 g 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
To determine the rate of reaction there are many method to be used for example, measuring the mass after the product has been added and measuring the difference in mass on the duration of a digital scale. Another method, which will be used in this experiment is using a gas syringe to measure the volume of the gas which has been produced. The cylinder inside, will be pushed out to show a quantitative presentation of the volume produced by the reaction. Hypothesis
As for the rock portion of the experiment, the students concluded that the mass percent of copper was 3.1%. This mass percent of Cu2+ is above the accepted value of 1.0 percent copper, which is the economically viable percent for mining copper ore. From this value of 1% copper in copper ore manufacturers can extract 9.99% pure copper (Copper Mining and Processing: What is Copper?, n.d.). These results show that the provided sample of copper ore would be worth mining, since it contains a higher percent of cu2+ than is needed to mine for copper. Overall, the experiment was accurate in determining the mass percent of cu2+ in the rock sample.
In cycle one, the double displacement reaction, Cu(s) + 4HNO3(aq) → Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) occurred, the result of the reaction was that the reaction mixture began to bubble with the copper filling dissolving and a vapor like substance leaving the reaction. Furthermore, when water was added, the color change, from brown to a blue color pigment. Then in Cycle two, another double displacement reaction occurred, Cu(NO3)2(aq) + 2NaOH(aq) → Cu(OH)2(s) + 2NaNO3(aq), which resulted in the reaction becoming cloudy and a darker shade of blue. Following cycle two, a decomposition reaction occurred as the result of heat being administered to the mixture, thus the following reaction occurred in cycle three, Cu(OH)2(s) → CuO(s) + H2O(l). As a