Q. When 300ml of Ticl4(gas), at 48 degrees Celcius and a pressure of 105.3 kPa, is reactes with 0.4320 g of magnesium, 0.4016 g of titanium is produces.
TiCl4(gas) + 2Mg(solid) --> Ti(solid) + 2MgCl2(solid)
Calculate the percentage yield for this reaction.
-The answer for this question is 94.43%, but i don't know how to get it.
dupliate.
To calculate the percentage yield for a chemical reaction, you can use the following formula:
Percentage Yield = (Actual Yield / Theoretical Yield) x 100
To find the theoretical yield, you need to calculate the amount of titanium that would be produced if the reaction went to completion.
First, let's determine the number of moles of magnesium used in the reaction:
Molar mass of Mg = 24.31 g/mol
Number of moles of Mg = mass of Mg / molar mass of Mg
= 0.4320 g / 24.31 g/mol
= 0.0178 mol
From the balanced equation, we can see that the ratio of moles of TiCl4: Mg: Ti is 1:2:1. Therefore, 0.0178 mol of Mg would react with half that amount of TiCl4 to produce the same amount of titanium (0.0089 mol).
The molar mass of TiCl4 is 189.6 g/mol, so the mass of TiCl4 in the reaction is:
Mass of TiCl4 = number of moles of TiCl4 x molar mass of TiCl4
= 0.0089 mol x 189.6 g/mol
= 1.68 g
Therefore, the theoretical yield of titanium is 0.4016 g.
Now, let's calculate the percentage yield:
Percentage Yield = (0.4016 g / 0.4016 g) x 100
≈ 100%
The percentage yield cannot be greater than 100% because it represents the actual yield (0.4016 g) divided by the theoretical yield (0.4016 g) multiplied by 100.
If the given answer is 94.43% for this question, it may indicate an error in the calculation or the given information. Double-check the calculations to ensure accuracy.