The balanced equation for the reaction of chromium metal and chlorine gas is 2Cr(s) + 3Cl2(g) → 2CrCl3(s) What is the limiting reactant when each of the following sets of quantities of reactants is mixed? (a) 4 Cr atoms and 6 Cl2 molecules (b) 6 Cr atoms and 10 Cl2 molecules (c) 12 Cr atoms and 20 Cl2 molecules

If 35g of LiCl mixes with 25g of Ca(OH)2, (a) which is the limiting reactant? (b) what is the theoretical yield? LiCl + Ca(OH)2 → LiOH + CaCl2

One of the commercial uses of sulfuric acid is in the production of calcium sulfate and phosphoric acid. If 26.8 g of Ca,(PO,), reacts with an excess of H,SO,, what is the percent yield if 13.4 g of H,PO, are formed in the following UNBALANCED chemical equation? Ca (PO,), (s) + H,SO, (aq) → H,PO, (aq) + CaSO, (aq)

Nitrogen (N2)and hydrogen (H2) react to form ammonia(NH3). Consider the mixture of N2 and H2 shown in theaccompanying diagram. The blue spheres represent N, andthe white ones represent H. (a) Write the balanced chemicalequation for the reaction. (b) What is the limiting reactant?(c) How many molecules of ammonia can be made, assumingthe reaction goes to completion, based on the diagram?(d) Are any reactant molecules left over, based on the diagram?If so, how many of which type are left over?

Balance the following chemical equation and determine the number of moles of Fe(s) produced when 1 moles of Fe2O3 (s) react with excess C(s) to produce Fe(s) and CO₂ (g). Fe2O3(s) + C(s) → Fe(s) + CO₂(g)

7.) A Sample Of 13.3g of Fe₂03 reacts with 16.89 CO со to yield Fe and Co₂. The balanced equation Fe₂O3 (s) + 3 C0g 2 Fe (5) + 300₂ (g) is Which Substance is the limiting reactant? What is the theoretical yield of Fe ? If the actual experimental yield for Fe is 8.41g what is the percent yield of Fe?

One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate.   Suppose an EPA chemist tests a 250.mL sample of groundwater known to be contaminated with iron(III) chloride, which would react with silver nitrate solution like this: FeCl3 (aq) + 3AgNO3 (aq) → 3AgCl (s) + FeNO33 (aq)The chemist adds 86.0m M silver nitrate solution to the sample until silver chloride stops forming. He then washes, dries, and weighs the precipitate. He finds he has collected 7.5mg of silver chloride.   Calculate the concentration of iron(III) chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits.

The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO,(G) + 0,(g) 2M1O,(G) + 2C0, (g) In the second step, manganese(IV) oxide and aluminum react to form manganese and aluminum oxidide: 3 MnO, (s) + 4Al(s) 3 Mn(s) + 2 Al,O3 (s) Suppose the yield of the first step is 95.% and the yield of the second step is 84.%. Calculate the mass of manganese(II) carbonate required to make 10.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. olo

A chemist invents a new combustion analysis instrument that uses less O2(g) which saves money on each analysis. The improvement is that instead of CO2(g) being formed and trapped, CO(g) is formed and trapped. H2O (g) is also formed and trapped when substances that contain hydrogen are analyzed.(a) The chemist places 2.184 g of an unknown compound of carbon and hydrogen in the new analyzer. 4.627 g of CO (g) and 1.795 g of H2O (g) are produced. Find the empirical formula for the compound.(Molar masses (g/mol): CO = 28.0104, H2O = 18.015) (b) Despite the best efforts of the chemist, the molar mass of the compound cannot be determined (using this method). Clearly explain why this prevents the determination of the molecular formula

Sand is mainly silicon dioxide. When sand is heated with an excess of coke (carbon),pure silicon and carbon monoxide are produced.(a) Write a balanced equation for the reaction.(b) How many moles of silicon dioxide are required to form 20.00 g of silicon?(c) How many grams of carbon monoxide are formed when 98.76 g of silicon areproduced?