In which case is O₂ the limiting reactant for 2H₂(g) + O₂(g) → 2H₂O(l)? 1 mol H₂, 2 mol O₂ 1 mol H₂, 1 mol O2 1 mol H₂, 3 mol O2 2 mol H₂, 1 mol O2 3 mol H₂, 1 mol O₂

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe (s)  +   CuSO4 (aq)  →   Cu (s)  +   FeSO4 (aq)Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a  350.mL  copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of  73.mg .   Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits. gL

following reaction is called BaCl₂ (aq) + K₂SO4 (aq). O single displacement reaction O precipitation reaction. O acid-base reaction Odouble displacement reaction BaSO4 (s) + 2KCl (aq)

1. Write the net ionic equation for the reaction. Show all the steps.  2. Do you expect the N-O bond in NO3- or NO to have a higher bond energy? Use Lewis structures to support your selection.

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO4(aq) → Cu(s) + FeSO4(aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 200. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 107. mg. Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits. 0 x10 х §

What mass in grams of iron metal can be formed by the reaction of 2.14 g Al metal with excess Fe₂O₃, according to the thermite reaction:     2 Al(s) + Fe₂O₃ → 2 Fe(s) + Al₂O₃(s)

A titration is performed to determine the amount of sulfuric acid, H2SO4, in a 6.5 mL sample taken from car battery. About 50 mL of water is added to the sample, and then it is titrated with 43.37 mL of a standard 0.5824 molar NaOH solution. You balanced this reaction in a previous problem. How many moles of sulfuric acid are present in the original sample?

The balanced equation below shows a simple way of manufacturing hydrogen gas in lab (you've done this!). For your convenience, the molar mass of each substance is shown below their formulas (in purple). Use this information to make the requested calculation: 2 Al(s) + 6 HCI(aq) -> 2 AICI3(aq) + 3 H2(g) 26.982 36.461 133.341 2.016 What volume of hydrogen gas, in L, will be produced by the reaction of 2.54 g of aluminum metal in excess hydrochloric acid?

What type of reaction is this? 2K(s) + Cl:(g) → 2KCI(s) * Synthesis Decomposition Combustion Single Replacement O Double Replacement

Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s)+2HCl(aq)→FeCl2(s)+H2S(g)FeS(s)+2HCl(aq)→FeCl2(s)+H2S(g) A reaction mixture initially contains 0.216 molmol FeSFeSand 0.660 molmol HClHCl Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?