Nitrogen and oxygen form an extensive series of oxides with the general formula NxOy. One of them is a blue solid that comes apart, reversibly, in the gas phase. It contains 36.84% N. What is the empirical formula of this oxide?

Copper(II) sulfate forms several hydrates with the general formula CuSO4·xH2O, where x is an integer. If the hydrate is heated, the water can be driven off, leaving pure CuSO4 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 31.%. Which hydrate is it? That is, what is x?

2a. Calculate the volumes of ammonia and oxygen required to produce 28 moles of nitrogen dioxide. 4NH3(g)+7O2(g)→4NO2(g)+6H2O(l) 2b. What is the mass of nitrogen dioxide produced if the yield is 88%?

a sample of solid silver oxide with a mass of 11.4 grams was reduced to elemental silver by heating under a flow of methane gas CH4- the reaction produced 10.6 grams of silver. what is the empirical formula of silver oxide?

Consider the following balanced chemical reaction: N2 (g) + 3 H2 (g) → 2 NH3 (g) What is the maximum mass (in grams) of ammonia (NH3) that can be produced from 9.36 g of N2 and 4.92 g of H2?

Combustion analysis of 2.796 g of an unknown compound containing carbon, hydrogen, and oxygen produced 5.597 g of CO2 and 2.268 g of H2O. What is the empirical formula of the compound?

8.40 g of hydrated nickel (II) sulfate is heated to produce 4.60 g of anhydrous compound NiSO4. Calculate the number of moles of anhydrous nickel (II) sulfate. Calculate the number of moles of water lost. What is the empirical formula of the hydrate?

1.  What is the mass percent composition of oxygen in a compound having the empirical formula C16H24O5? 2. Nitrous oxide (N2O) having a mass of 4.14 g reacts completely with an equimolar amount of NO2 to form elemental nitrogen and oxygen. What is the mass of N2 formed in this reaction? 3.  If 61.0 mL of KCl(aq) solution is combined with 90.0 mL of 0.500 M AgNO3, a white solid identified as AgCl(s) precipitates from the solution. After filtering and weighing, the mass of AgCl was determined to be 0.890 g. What was the original concentration of the KCl solution?

A molecular formula expresses the number of each kind of atom in a molecule. For example, the molecular formula for propene, C3H6C3H6, indicates three carbon atoms and six hydrogen atoms per molecule. This also means that one mole of propene contains three moles of carbon and six moles of hydrogen.An empirical formula expresses the mole ratio of the elements. The empirical formula for propene is CH2CH2, indicating twice as much hydrogen as carbon. When analyzing unknown compounds in a lab, it is often possible to identify the mole ratios, and thus the empirical formula, but not the molecular formula.Notice that the molecular mass of propene, 3(12)+6(1)=42amu3(12)+6(1)=42amu, is a multiple of the empirical formula mass, 1(12)+2(1)=14 amu An unknown compound contains only carbon, hydrogen, and oxygen (CxHyOzCxHyOz). Combustion of 6.50 gg of this compound produced 9.53 gg of carbon dioxide and 3.90 gg of water. Part A How many moles of carbon, CC, were in the original sample?…

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