Answer:
Step-by-step explanation:
To calculate the percent yield of a reaction, we need to compare the actual yield (the amount of product obtained in the experiment) with the theoretical yield (the amount of product that should have been obtained based on stoichiometric calculations).
The balanced chemical equation for the reaction between magnesium bromide (MgBr2) and hydroiodic acid (HI) is:
MgBr2 + 2HI → MgI2 + 2HBr
From this equation, we can see that 1 mole of MgBr2 reacts with 2 moles of HI to produce 1 mole of MgI2 and 2 moles of HBr. We can use this information to calculate the theoretical yield of HBr that should have been obtained based on the amount of MgBr2 used:
Calculate the moles of MgBr2 used:
moles of MgBr2 = mass / molar mass = 24.5 g / 184.11 g/mol = 0.133 moles
Use the mole ratio from the balanced equation to calculate the moles of HBr that should have been produced:
moles of HBr = 2 x moles of MgBr2 = 2 x 0.133 moles = 0.266 moles
Calculate the mass of HBr that should have been produced:
mass of HBr = moles of HBr x molar mass = 0.266 moles x 80.91 g/mol = 21.47 g
So the theoretical yield of HBr is 21.47 g.
The actual yield of HBr obtained in the experiment is 8.23 g.
We can now calculate the percent yield as:
percent yield = (actual yield / theoretical yield) x 100%
percent yield = (8.23 g / 21.47 g) x 100%
percent yield = 38.4%
Therefore, the percent yield of the reaction is approximately 38.4%.