Question

3a) Nickel(II) oxide reacts with carbon to produce nickel metal and carbon dioxide gas. How many grams of nickel would be produced from the reaction of 50.0 grams of nickel(II) oxide and 10.0 grams carbon, if the reaction is 75% successful? b) If the reaction were only 60% successful, how many grams of nickel(II) oxide and carbon would be required to actually produce 500 grams of nickel metal by the reaction?

Answer 1

The balanced equation is 2NiO+ C--->2Ni+CO2

Molarmass (g/mol) 157. 12. 141

(a)2 mol=2*157g of NiO reacts with 1 mol= 12 g of C

50 g of NiO reacts with (50*12)/(2*157)= 1.91 g of C

So 10.0-1.90= 8.09 g of C left unreacted and is excess reactant

Since all of NiO completely reacted it is limiting reactant.

2*157 g of NiO produces 2 mol= 2*141 g of Ni

50.0 g of NiO produces (50.0*2*141)/(2*157)=44.9 g of Ni

This is for 100 % it is 44.9 g

For 75% the product formed is (44.9*75)/100=33.7 g