PLEASE PLEASE PLEAS HELP ME WITH THIS, ITS DUE TOMORROW 03/02/2021 AND IM SO LOST. 50% of grade 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?

b. is the answer hoped i        

answer : (a) volume of the gas = 8.67 ×   l

                (b) second virial coefficient b = -1.21226 l/mole

solution :   given,     t = 300k

                                p = 20atm

                                z = 0.86

                                n = 8.2 mmoles = 8.2 × moles

                                r =   0.082 l atm/k/mol

        find,     (a) volume of gas   and (b) second virial coefficient b at 300k.

formula used :            

                          and            

(a)            

                    = \times 0.082\times 300}{20}[/tex]

                    = 8.67 ×   l

(b)      

                    = (0.00867-1) × 8.659

                    = - 8.5839 l/mole

the answer is a for sure mark brainliest i had got this right on usatestprep

it's