Copper in Silver Nitrate Lab

In this experiment, we learned about stoichiometry, empirical formula, molecular formula, polyprotic acids and bases, metathesis reactions, and moles.

The purpose of this lab was to determine the limiting reactant in a mixture of to soluble salts and the percent composition of each substance in a salt mixture.

It is a chemical reaction where the colors of both solution and iron strip changed. It is

The purpose of the experiment is to cycle solid copper through a series of five reactions. At different stages of the cycle, copper was present in different forms. First reaction involves reaction between the copper and nitric acid, and copper changed from elemental state to an aqueous. The second reaction converted the aqueous Cu2+ into the solid copper (2) hydroxide. In the third reaction Cu(OH)2 decomposed into copper 2 oxide and water when heated. When solid CuO reacted with sulfuric acid, the copper returned to solution as an ion (Cu2+). The cycle of reactions was completed with the reaction where elemental copper was regenerated by Zn and Cu

and Cl - . If Ag + was present instead, then the solution would have consisted of silver chloride

1. Suppose that you have an unlimited supply of copper (II) sulfate to react with iron. How many moles of copper would be

12. Write the balanced chemical reaction of the product of the reaction described above (problem 11) with NaOH. Is the product of this reaction soluble in aqueous solution?

The purpose of this lab was to determine the limiting reactant in a reaction between copper sulfate and iron. Using the reaction between copper sulfate and iron, the reaction was observed to see the reaction and transformation of matter. The copper sulfate was placed into a beaker, as the excess reactant, then iron filings added until the heated solution was completely reacted. This reaction created an excess of leftover. The law of conservation of mass can be observed in this reaction, and using the data found, the percent yield calculated.

Purpose: The purpose of this experiment is to observe a variety of chemical reactions and to identify patterns in the conversion of reactants into products.

-If the copper metal is submerged in the silver nitrate solution then in reaction, a pure, solid (Ag) silver product is created with an excess of (Cu (NO3)2) copper (II) aqueous liquid because a single displacement reaction occurs where the balance equation is then

I started with elemental copper metal and then reactions occur step by step as follows:

Experimental approach: In the first reaction, copper metal turnings oxidize when put in contact with nitric acid and become copper nitrate.

The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was found to be 2.1726g which meant that through limiting reagent analysis Fe was determined to be the limiting reagent and the chemical reaction was determined to be as following:-

The main purpose of this experiment was to show that single displacement reactions between metals according to their reactivity, with more reactive elements having the power to displace less reactive elements and take their place in a chemical compound (Beran, 2014). This was supported by the results of the experiment, where solid metals were combined with aqueous solutions that contained another element, and reactions only took place when the solid metal was more reactive than the other element in the compound. Only three attempted trials resulted in a failure to produce a reaction, namely the combinations of copper with hydrochloric acid, and copper with nickel sulfate. The outcomes of these trials are justifiably reasonable because copper is ranked lower in the

The purpose of the experiment is to obtain silver nanoparticles from the reduction reaction between silver nitrate and sodium borohydride. Silver atoms are aggregated after silver nitrate was reduced by sodium borohydride, with the aid of sodium citrate to manipulate the sizing of silver nanoparticles. Without sodium citrate, bulky, ununiformed precipitates will begin to form without control. Hydrogen peroxide served as an oxidizing agent to balance out the reduction of sodium borohydride and oxidation of hydrogen peroxide. Hydrogen peroxide & sodium borohydride shall not react particularly in this experiment. Typically, when those two reagents react, H2 gas will form. There was no sign of bubbles produced during the reduction experiment, mostly dependent on the quantity used and procedure of chemical mixing. There was presence of other chemicals within the solution, which reduces the probability of reaction occur between two reagents.