A student is given a 1.3308 g of an unknown copper compound. Following isolation by displacement by Mg, 0.5830 g of Cu metal is recovered. What is the percentage of Cu in the sample? You may assume that one mole of the sample contains one mole of copper.

1)Copper metal reacts with molecular nitrogen to form copper(II) nitride.  a)Write the balanced chemical equation for this reaction.  Please be sure to include the physical state of each substance as well.  b) If 81.0 g of copper reacts with 16.8 g of molecular nitrogen, what is the maximum amount of copper(II) nitride (in GRAMS) that could be produced?

Lead(II) oxide from an ore can be reduced to elemental lead by heating in a furnace with carbon. Calculate the expected yield of lead if 67.0 kg of lead oxide is heated with 67.0 kg of carbon.

A student determined the mass of NaCl extracted during an experiment to be 0.42 grams. If the mass of the original mixture was 1.97 determine the percent of NaCl.

During a laboratory experiment, a student initiated a reaction with 19.5 g of NaBH4 and excess BF3. When the reaction was complete, the student had collected 7.00 g of B2H6 gas. From this data, calculate the percent yield of B2H6.

Part A A sample of 7.92 g of Mg(OH)2 is added to 24.2 mL of 0.225 MΗΝΟ, Part B Part C • Part D • Part E How many moles of Mg(NO3)2 are present after the reaction is complete? Express your answer in moles to three significant figures.

00 S Nazza .01608 ·018302 3. (part a). You are given 0.104 g of a sample of KwFex(C₂O4)y(H₂O)z. In the laboratory, you titrate this sample with 0.00940 M KMnO4 and you need 10.1 mL of the KMnO4 solution to reach the stoichiometric point. Calculate the mass and moles of [C₂04]²- in the sample. Please show all of your detailed calculations.

A 235.2-g sample of ground water is analyzed for calcium. The Ca2+ in the sample is first precipitated and filtered-off as NH4CaPO4·7H2O. This precipitate is dried and heated, releasing water and ammonia to yield anhydrous calcium pyrophosphate (Ca2P2O7). The mass of Ca2P2O7 obtained is 0.0234 g.Give the calcium content of the ground water in parts per million (to three significant figures).

A 290.3-g sample of ground water is analyzed for calcium. The Ca2+ in the sample is first precipitated and filtered-off as NH4CaPO4·7H2O. This precipitate is dried and heated, releasing water and ammonia to yield anhydrous calcium pyrophosphate (Ca2P2O7). The mass of Ca2P2O7 obtained is 0.0534 g.Give the calcium content of the ground water in parts per million

An impure sample of table salt (NaCl) that was dissolved in water and treated with silver nitrate to form silver chloride. If the initial sample had a mass of 1.741 g and the final mass of the AgCl was found to be 4.084 g, what is the mass percent of NaCl in the impure sample?