Iron metal is produced from the mineral hematite (Fe2O3) and pure carbon, as given by the equation: Fe2O3 (s) + C (s)  -> Fe (s) + CO2 (g) [unbalanced]

Balance this equation. Then, use the mole ratios therein to perform the calculations below.

a. How many moles of C are required to completely react with 14.251 moles of Fe2O3 (hematite)?

b. How many moles of Fe2O3 must react to generate 0.986 moles of pure iron?

c. How many moles of CO2 will be generated if 2.774 moles of carbon completely reacts?

d. What is the limiting reactant?

e. Calculate the mass of excess reactant that remains when the reaction is complete.

f. When this reaction is performed in the laboratory, the percent yield of CO2 is 72.6%. What was the experimental yield of CO2?

A3.37-mg sample of protein was chemically digested to convert its nitrogen into ammonia and then diluted to 100.0 ml. then 10.0 ml of this solution was placed in a 50-ml volumetric flask and treated with 5 ml of phenol solution plus 2 ml of sodium hypochlorite solution. the sample was diluted to 50.0 ml, and the absorbance at 625 nm was measured in a 1.00-cm cuvette and found to be 0.486. for reference, a standard solution was prepared from 10.0 mg of nh4cl (molar mass = 53.49 grams/mole) dissolved in 1.00 l of water. then 10.0 ml of this standard was placed in a 50-ml volumetric flask, treated in the same manner as the unknown, and the absorbance found to be 0.323. finally, a reagent blank was prepared using distilled water in place of unknown, it was treated in the same manner as the unknown, and the absorbance found to be 0.076. calculate the weight percent of nitrogen in the protein.

If i can still dissolve more sugar into the solution at a certain temperature what would i call that solution

Which substance can be broken down by chemical means