Step-by-step explanation:
1. First, let's rewrite the equation:
FeO + H2O --> Fe(OH)2
1 mole of FeO react with one mole of H2O producing 1 mole of Fe(OH)2.
Let's transform 1000g of FeO and 800 g of H2O into moles using: n = m/MM
MM of FeO = 72 g/mol
MM of H2O = 18 g/mol
n FeO = 1000/72
n FeO = 13.89 moles
n H2O = 800/18
n H2O = 44.4 moles
We can see that we have less moles of FeO than of water. The ratio between them is 1:1, so FeO is our limiting reactant.
Answer 1: FeO is the limiting reactant.
2. To calculate the theoretical yield, we need to use the number of moles of the limiting reactant, which is 13.89.
So it will be produced 13.89 moles of Fe(OH)2, since the ratio between FeO and Fe(OH)2 is 1:1.
So let's transform 13.89 moles of Fe(OH)2 into grams:
m = n*MM
MM of Fe(OH)2 = 90 g/mol
m = 13.89*90 = 1250.1 g of Fe(OH)2
Answer 2: Theoretical yield = 1250 g of Fe(OH)2
4. The excess reactant is H2O.
After the reaction, it will left 44.4 - 13.89 = 30.51 moles of H2O.
It is in grams:
m = n*MM
m = 30.51*18
m = 549 g
Answer: 549 g