is it easy to distinguish between between the different oxidation states of copper? why?
-I answered yes because copper (I) is not as stable as copper (II), and there is a noticeable colour difference
You synthesized copper (I) chloride and copper (I) oxide. How do they differ from their copper (II) analogs? comment on the stability of these moist solids in air. If unstable, what is the likely product of decomposition?
-I'm not really sure where to go with this one, would it be something along the line of copper (II) is more stable than copper (I)?
calculate the percent recovery of copper from 10 mL of .10M of Cu(NO3)2? (how would you do this question?)
Percent recovery: Moles = Concentration * Volume .10 M * 10 mL = .10 M * .010 L = .001 mol Percent recovery = ((# of moles) * (molar mass of copper)) = .063546/.0191g =30 percent recovery
Is it necessary to synthesize the various copper compounds in order to recover copper metal?
I answered no, the metal can be extracted using less steps but the metal wont be as pure as it is using all the stpes
Also, how can you write word equations for reactions? For example, adding HCl to CuO.
For the question "Is it necessary to synthesize the various copper compounds in order to recover copper metal?", I would explain that it is not necessary to synthesize the various copper compounds in order to recover copper metal. Copper can be obtained through other methods, such as smelting or electrolysis, which involve extracting copper from its ores or compounds. These methods result in the production of impure copper, but purification techniques can be employed to obtain pure copper.
Regarding writing word equations for reactions, you typically start with the reactants on the left side of the equation and the products on the right side, separated by an arrow. For example, the reaction of adding hydrochloric acid (HCl) to copper oxide (CuO) can be written as:
CuO + 2HCl → CuCl2 + H2O
In this reaction, copper oxide reacts with hydrochloric acid to produce copper chloride and water. The numbers in front of the chemical formulas (coefficients) indicate the stoichiometric ratio of the reactants and products. In this case, 1 mole of copper oxide reacts with 2 moles of hydrochloric acid to produce 1 mole of copper chloride and 1 mole of water.