Answer:
1. The theoretical yield of NiO is 5.09g.
2. O2 is the limiting reactant.
3. The percentage yield of NiO is 95.5%
Step-by-step explanation:
Step 1:
The balanced equation for the reaction is given below:
2NiS2(s) + 5O2(g) —> 2NiO(s) + 4SO2(g)
Step 2:
Determination of the masses of NiS2 and O2 that reacted and the mass of NiO produced from the balanced equation. This is illustrated below below:
Molar mass of NiS2 = 59 + (32x2) = 123g/mol
Mass of NiS2 from the balanced equation = 2 x 123 = 246g
Molar mass of o3= 16x2 = 32g/mol
Mass of O2 from the balanced equation = 5 x 32 = 160g
Molar mass of NiO = 59 + 16 = 75g/mol
Mass of NiO from the balanced equation = 2 x 75 = 150g
Summary:
From the balanced equation above, 246g of NiS2 reacted with 160g of O2 to produce 150g of NiO
Step 3:
Determination of the limiting reactant. This can be obtain as follow:
From the balanced equation above, 246g of NiS2 reacted with 160g of O2.
Therefore, 11.2g of NiS2 will react with = (11.2 x 160)/246 = 7.28g of O2.
From the above calculation, we can see that it will take a higher mass of O2 i.e 7.28g than what was given i.e 5.43g to react completely with 11.2g of NiS2.
Therefore, O2 is the limiting reactant and NiS2 is the excess reactant.
1. Determination of the theoretical yield of NiO.
In this case, the limiting reactant will be used as all of it is consumed in the reaction. The limiting reactant is O2.
From the balanced equation above, 160g of O2 reacted to produce 150g of NiO.
Therefore, 5.43g of O2 will react to produce = (5.43 x 150)/160 = 5.09g of NiO.
Therefore, the theoretical yield of NiO is 5.09g.
2. The limiting reactant is O2. Please review step 3 above for explanation.
3. Determination of the percentage yield of NiO. This is illustrated below:
Actual yield of NiO = 4.86g
Theoretical yield of NiO = 5.09g
Percentage yield =..?
Percentage yield = Actual yield /Theoretical yield x 100
Percentage yield = 4.86/5.09 x 100
Percentage yield of NiO = 95.5%