You are given a sample that contains a mixture of the following two arsenic-containing minerals: gersdorffite (NiAsS) and getchellite (AsSbS3). You start with a sample of this mixture that has a mass of 57.38 grams. You perform a reaction that converts the arsenic (As) in these minerals into the form arsenic(V) oxide (As2O5), and 36.03 grams of this product are obtained. What is the percent by mass of gersdorffite in the original sample?

Part A: What mass of water is produced when 10.5 g of hydrogen reacts with 100.0 g of oxygen? The chemical equation for this reaction is:  2H2(g)  +  O2(g) →  2H2O(g)  Part B: What mass of reactant(s) remains after the reaction is complete?

What mass of Cu(IO3)2 can be formed from 0.650 g of CuSO4 · 5H2O? What mass of KIO3 is needed to convert the copper in 0.2750 g of CUSO4 - 5H2O to Cu(IO3)2?

To help farmers and gardeners , commercial fertilizers have a big three -number "NPK" label on the bag that gives the amounts of three key plant nutrients: nitrogen , phosphorus and potassium. For example , a bag of "-10-10-10" fertilizer has 10% by mass nitrogen , 10% by mass potassium as potash (K2O), and 10% by mass phosphorus as phosphate (P2O5). Suppose a certain fertilizer has the following composition. What should the first (nitrogen) number on the bag label be? That is, calculate the the percent by mass of nitrogen in this fertilizer. Round your answer to the nearest percent.

The formula for alum is KAl(SO4)2  x 12 H2O. All of the atoms in this formula contribute to the molar mass. When you add up all the masses in the formula, the molar mass is 474.39 grams/mole. The molar mass of aluminum is 26.98.   If you started this experiment with 1.063 grams of aluminum foil, what is the theoretical yield      of  Alum? Give your answer to 1 decimal place.  __________________________   The actual yield of alum in the lab was 17.8 grams. What percentage yield is this? Give your       answer to 1 decimal place.  ____________________________

Consider the following balanced equation. 3 Ag(s) + 4 HNO3(aq) → 3 AgNO3(aq) + NO(g) + 2 H2O(l) A student used 117.24 g of Ag and obtained 135.49 g of AgNO3, calculate the percent yield of AgNO3. Give your answer to the correct number of significant figures without unit. Molar mass of Ag: 107.87 g/mol Molar mass of HNO3: 63.01 g/mol Molar mass of AgNO3: 169.87 g/mol Molar mass of NO: 30.01 g/mol Molar mass of H2O: 18.02 g/mol

Lithium reacts with nitrogen to form lithium nitride. 6 Li(s) + N2(g) → 2 Li3N(s) In one experiment 3.0 mole of Li is combined with 1.0 mole of N2. In another experiment 13.88 g of Li reacts completely with excess N2. What mass of Li3N (34.83 g mol–1) is formed?   11.6 g   23.2 g   55.6 g

Cobalt(II) chloride forms several hydrates with the general formula CoCl2 ·x H2O , where  x  is an integer. If the hydrate is heated, the water can be driven off, leaving pure  CoCl2  behind.   Suppose a sample of a certain hydrate is heated until all the water is removed, and it's found that the mass of the sample decreases by 22.% . Which hydrate is it? That is, what is  x ?

A student performed a similar experiment to the one you performed: They took a crucible and lid, cleaned them, heated them over a flame, and after cooling found their combined mass to be 22.538 g. The student then added a sample of zinc(II) sulfate hydrate (ZnSO4·“n”H2O) to the crucible so the combined mass of the sample, crucible, and lid was 25.896 g. They heated this sample for 10 minutes with the lid ajar, let it cool, and measured the mass of the crucible, sample, and lid to be 25.054 g. a. Based on this experiment, what is the formula for they hydrated zinc(II) sulfate compound? b. The student later looked on the reagent bottle for zinc(II) sulfate hydrate and found the actual formula was ZnSO4·7H2O. If everything had been done correctly, what value should the student have expected for the final mass of their sample, crucible, and lid after heating?

Carbon tetrachloride was prepared by reacting 23.6 g of carbon disulfide and 47 g of chlorine gas. CS2 + 3 Cl2 → CCl4 + S2Cl2 What mass of disulfur dichloride was produced?