2 student overachiever reported a final yield of 115% list two things he might have done wrong to account for this yield 10 lab report, hand in w ithin 24 hours 3 of the four copper compounds: cu(no3)2, cu(oh)2, cuo, cuso4, observed in this experiment, which two are the least soluble 4. Chemical transformations of copper introduction: in this experiment, a weighed amount of copper metal is transformed, through a series of reactions, into other copper-containing compounds, and is eventually returned to the metal state in part e of the experiment, the zinc metal is added to undergo a redox reaction with the copper(ii. In a laboratory experiment, h2(g) is collected over water in a gas-collection tube as shown in the diagram above the temperature of the water is 21°c and the atmospheric pressure in the laboratory is measured to be 772 torr.
So, here , on adding zinc to cuso4 solution, zinc displaces copper from copper sulphate & forms zinc sulphate solution this is indicated by colour change from blue to colourless cuso4 solution has a blue colour while znso4 solution is colourless. The initial mass of copper used in the experiment was 2004 grams, and the initial moles of copper was 00315 due to the law of conservation of mass, one would predict that after any number of chemical reactions and phase changes, the final mass and number of moles of copper would remain the same as the initial amounts.
The yield of copper was too high in this experiment 1955g of cu was given, but 546g of cu was recovered in the conclusion the percent yield turn out to be 288%, 188% away from the theoretical yield. Chemistry - nchs lab: reactions of copper and percent yield page 1 of 8 the objective in this experiment is to recover all of the copper you begin with in analytically pure form this is the test of your laboratory skills. Through various chemical reactions, recovered mass of copper is found to be larger than initial mass of copper 1955g of cu was given initially 564g of cu was produced if the lab was accurately done, the amount of copper that was left over should have theoretically weighed the same as the weight of initial copper.
Ap chem final study play in a laboratory experiment, h2(g) is collected over water in a gas-collection tube as shown in the diagram above the temperature of the water is 21°c and the atmospheric pressure in the laboratory is measured to be 772 torr what number of moles of o2 is needed to produce 142 grams of p4o10 from p. Demonstration in this experiment copper(ii) oxide and zinc metal are reacted together the reaction is exothermic and the products can be clearly identified the experiment illustrates the difference in reactivity between zinc and copper and hence the idea of competition reactions. Copper levels in muscle, kidney, and organs of rainbow trout were approximately 08-11, 20-23, and 115-150 mg/kg fresh weight, respectively, after 12 months intermittent exposure to various copper sulfate containing formulations 06, 20, and 100 mg/kg, respectively, in controls . Molarity = moles copper / liter solution moles of copper = grams of copper / molecular weight of copper 2 from the announced molarity of the copper nitrate solution (not your calculated molarity) and the volume of solution that was used, calculate the theoretical yield (in grams) of copper. A tolerance is established in potable water for residues of copper resulting from the use of the algicides or herbicides basic copper carbonate (malachite), copper sulfate, copper monoethanolamine, and copper triethanolamine to control aquatic plants in reservoirs, lakes, ponds, irrigation ditches, and other potential sources of potable water.
The interaction of the hydrochloric acid and zinc is called an oxidation-reduction reaction it is also referred to as a redox reaction this type of reaction involves an exchange of electrons between two elements.
3(2 points) based on the balanced equations of question 1, if you used 850 mg of copper in the initial reaction, calculate the exact amount of zinc required to complete the reaction in equation d. Finally, zinc metal reduces the hydrated copper (ii) ion back to metallic copper while itself turning being oxidized to zinc (ii) ions we have seen this reaction before in the copper chloride lab .