Answer:
Balanced reaction:
3MgO + 2Fe -> 3Mg + Fe2O3
11.3 g of MgO are needed to produce 15 g of Fe2O3
Explanation:
The balanced reaction is:
3MgO + 2Fe -> 3Mg + Fe2O3
Ratio is 1:3. First of all we determine the moles of produced oxide.
15 g . 1mol / 159.7 g = 0.0939 moles.
Now, the rule of three:
1 mol of oxide was produced by 3 moles of MgO
Then, 0.0939 moles of oxide were produced by 0.282 moles.
If we convert the moles to mass, we will get the answer 0.282 mol . 40.3g / 1mol = 11.3 g
Answer:
We need 11.35 grams of MgO
Explanation:
Step 1: Data given
Mass of Fe2O3 = 15.0 grams
Molar mass Fe2O3 = 159.69 g/mol
Step 2: The balanced equation
3MgO(s) + 2Fe(s) → Fe2O3(s) + 3Mg(s)
Step 3: Calculate moles Fe2O3
Moles Fe2O3 = mass Fe2O3 / molar mass Fe2O3
Moles Fe2O3 = 15.0 grams / 159.69 g/mol
Moles Fe2O3 = 0.0939 moles
Step 4: Calculate moles MgO
For 3 moles MgO we need 2 moles Fe to produce 1 mol Fe2O3 and 3 moles Mg
For 0.0939 moles Fe2O3 we need 3* 0.0939 = 0.2817 moles MgO
Step 5: Calculate mass MgO
Mass MgO = moles MgO * molar mass MgO
Mass MgO = 0.2817 moles * 40.30 g/mol
Mass MgO = 11.35 grams
We need 11.35 grams of MgO
