the balanced molecular equation for the replacement reacttion that occurs betwee

Question

the balanced molecular equation for the replacement reacttion that occurs between solid iron (III) oxide and solid carbon is 2Fe2O3(s)+3C(s) =4Fe(s) + 3CO2(g). Given that the furnace starts wirh 1.00kg of carbon

A) how many moles of iron would you produce?

B) given that the chemist starts with 1.00kg of iron (III) oxide, how many moles of iron would you produce?

C) Which is the limiting reactant? 1..iron (III) oxide, 2..carbon.. 3 iron 4/both 1 and 2

D) Whats the theoretical yield in KG?

E) THE CHEMIST actually produces 500.00g of product. What is the percent yiels?

Explanation / Answer

mol C= mass/MW = 1000/12 = 83.333 mol of C

then, expect

3:4 ratio = 4/3*83.333 = 111.1106 mol of Fe

mass = mol*MW = 111.1106 *55.5 = 6166.63 g of Fe = 6.16 kg of Fe

b.

mol Fe2O3 = 1000/159.69 = 6.2621

ratio is 2:4

so

6.2621*2 = 12.5242 mol of Fe

c.

limiting is Fe2O3

d.

yield

6.16 kg of Fe

e.

% yield = 5 / 6.16 * 100 = 81.1688 %

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