Study the balanced equation.
3Mg + Fe2O3 → 3MgO + 2Fe
What is the theoretical yield for MgO when 0.52 mol of Mg and 0.28 mol of Fe2O3 react?
2.10 x 101 mol MgO
1.03 x 101 mol MgO
2.10 x 101 g MgO
3.39 x 101 g MgO
3Mg + Fe2O3 → 3MgO + 2Fe
The limiting reagent (LR) must be determined.
0.52 mols Mg x (3 mol MgO/3 mol Mg) = 0.52 mol MgO or
0.28 mols Fe2O3 x (3 mol MgO/1 mol Fe2O3) = 0.84 mols MgO so Mg is the LR and it will produce as a theoretical yield 0.52 mols MgO.
So neither a nor b are correct for mols. Try grams.
molar mass MgO is 40.3 so grams MgO produced at 100% yield wil be
40.3 x 0.52 = 21 rounded to 2 places so you pick answer c.
Anyone?
Ah, the wonderful world of theoretical yields! Let's calculate it, shall we?
According to the balanced equation, the molar ratio between MgO and Mg is 3:3. So, for every 3 moles of Mg, we can expect 3 moles of MgO.
Now, let's do some math. If we have 0.52 moles of Mg, we can set up a proportion:
0.52 mol Mg / 3 mol Mg = x mol MgO / 3 mol MgO
Cross-multiplying, we get:
(0.52 mol Mg)(3 mol MgO) = 3 mol Mg(3 mol MgO)
1.56 mol MgO = 9 mol MgO
So, the theoretical yield for MgO is 1.56 moles. But wait, there's more!
Now, let's calculate the molar ratio between MgO and Fe2O3. According to the balanced equation, it's 3:2. So, for every 2 moles of Fe2O3, we can expect 3 moles of MgO.
If we have 0.28 moles of Fe2O3, we can set up another proportion:
0.28 mol Fe2O3 / 2 mol Fe2O3 = x mol MgO / 3 mol MgO
Cross-multiplying again, we get:
(0.28 mol Fe2O3)(3 mol MgO) = 2 mol Fe2O3(x mol MgO)
0.84 mol MgO = 2 mol Fe2O3(x mol MgO)
So, the theoretical yield for MgO based on Fe2O3 is 0.84 moles.
Now, to find the overall theoretical yield, we can simply add up the two yields:
1.56 moles (from Mg) + 0.84 moles (from Fe2O3) = 2.40 moles
The theoretical yield for MgO is 2.40 moles.
And finally, to answer your question (I haven't forgotten!), none of the given options match the calculated theoretical yield. So, I'm afraid I can't provide a suitable answer. But hey, at least we had some fun with math!
To determine the theoretical yield for MgO, we need to use the balanced equation and the given amounts of reactants.
According to the balanced equation:
3Mg + Fe2O3 → 3MgO + 2Fe
The molar ratio between MgO and Fe2O3 is 3:1, meaning that for every 3 moles of MgO produced, 1 mole of Fe2O3 is consumed.
Given:
0.52 mol of Mg
0.28 mol of Fe2O3
From the reaction, we can see that the ratio of MgO to Fe2O3 is 3:1.
Therefore, the moles of MgO formed when 0.28 mol of Fe2O3 is consumed can be calculated as:
0.28 mol Fe2O3 x (3 mol MgO / 1 mol Fe2O3) = 0.84 mol MgO
So, the theoretical yield for MgO is 0.84 mol.
The correct answer is 0.84 mol MgO (option 2).
To determine the theoretical yield of MgO (magnesium oxide), we need to use the balanced equation and stoichiometry.
Let's start by examining the coefficients in the balanced equation:
3Mg + Fe2O3 → 3MgO + 2Fe
This equation tells us that 3 moles of Mg react with 1 mole of Fe2O3 to produce 3 moles of MgO.
From the given information, we have 0.52 mol of Mg and 0.28 mol of Fe2O3. To determine the limiting reactant (the reactant that will be completely consumed and determine the amount of product formed), we need to compare the mole ratios of the reactants.
For Mg:
0.52 mol Mg x (3 mol MgO / 3 mol Mg) = 0.52 mol MgO
For Fe2O3:
0.28 mol Fe2O3 x (3 mol MgO / 1 mol Fe2O3) = 0.84 mol MgO
Since the stoichiometric ratio is 1:1 for Mg and Fe2O3, the limiting reactant is Mg because it produces fewer moles of MgO.
Now, we can convert the moles of MgO to grams using its molar mass:
Molar mass of MgO = 24.31 g/mol (Mg) + 16.00 g/mol (O) = 40.31 g/mol
0.52 mol MgO x (40.31 g MgO / 1 mol MgO) = 20.97 g MgO
Therefore, the theoretical yield of MgO is 20.97 g MgO.
Among the given options:
2.10 x 10^1 mol MgO is not correct because it does not match the calculated value.
1.03 x 10^1 mol MgO is not correct because it does not match the calculated value.
2.10 x 10^1 g MgO is not correct because it does not match the calculated value.
3.39 x 10^1 g MgO is not correct because it does not match the calculated value.
So none of the options provided are correct. The correct answer is 20.97 g MgO.