2 Mg (s) + O2 (g) → 2 MgO (s)
4.00mg x 1 mol Mg/24.305 x 2 mol MgO/2 mol Mg x 40.305g MgO/1 mol MgO=
=6.63g
4.00g- Given
24.305g- Atomic Mass of Magnesium
40.305g- Atomic Mass of Magnesium Oxide
Magnesium chloride: 81,95 g are obtained.
You must first calculate the theoretical yield of your product using the balanced equation. The crude yield is divided by the theoretical yield and multiplied by 100.
The percentage yield is the Actual Yield divided by the Theoretical Yield, all multiplied by 100. Percentage = [(Actual)/(Theoretical)] x 100
No, competing side reaction is a reson why the actual yield is more than the theoretical yield.
# Determine the limiting reagent; # Calculate the expected yield if the reaction goes to 100% completion. # Divide the actual yield by the expected yield and multiply by 100. The result is percentage yield.
The theoretical yield is 56,7 %.
The actual yield is 73 %.
1,7 mol oxide
Use pure magnesium and pure oxygen.
A theoretical yield is equivalent to a percent yield of 100. In practice, it is very rare to achieve 100 yield from a reaction due to a wide range of outside factors 1.7mol
Magnesium chloride: 81,95 g are obtained.
1.30
2,55 moles of aluminium oxide are obtained.
1.60mol
Theoretical= calculated
The actual yield is less than the theoretical yield.
Magnesium is extracted from its ores by one of two processes. In the first, the ore is converted to magnesium chloride (MgCl2), which is then electrolyzed. In the second process, the ore is converted to magnesium oxide (MgO), which is then treated with the alloy ferrosilicon. The ferrosilicon reacts with magnesium oxide to yield pure magnesium metal.It is the same for potassium, they both need to be electrolyised