A student dehydrated 12 grams of 2-methylcyclohexene with 85% H3PO4, and acquired 6.50 grams of alkene. What are the theoretical and percent yields?
To determine the theoretical yield and percent yield, we need to understand the reaction taking place and use a balanced chemical equation.
The reaction being described is the dehydration of 2-methylcyclohexanol to form 2-methylcyclohexene. The balanced chemical equation for this reaction is:
2-methylcyclohexanol ---> 2-methylcyclohexene + H2O
From the equation, we can see that one mole of 2-methylcyclohexanol reacts to produce one mole of 2-methylcyclohexene.
First, we need to determine the number of moles of 2-methylcyclohexanol. We can calculate this using the given mass and the molar mass of 2-methylcyclohexanol.
Molar mass of 2-methylcyclohexene = 84.16 g/mol
Number of moles of 2-methylcyclohexene = mass / molar mass
= 6.50 g / 84.16 g/mol
= 0.0773 mol
Since the reaction is 1:1, the number of moles of 2-methylcyclohexanol is also 0.0773 mol.
Now, the theoretical yield can be calculated by multiplying the number of moles of 2-methylcyclohexene by its molar mass:
Theoretical yield = number of moles of 2-methylcyclohexene * molar mass of 2-methylcyclohexene
= 0.0773 mol * 84.16 g/mol
= 6.50 g
So, the theoretical yield is 6.50 grams.
Next, we can calculate the percent yield by using the formula:
Percent yield = (actual yield / theoretical yield) * 100
Given that the actual yield is 6.50 grams and the theoretical yield is also 6.50 grams:
Percent yield = (6.50 g / 6.50 g) * 100
= 100%
Therefore, the percent yield is 100%.
In summary, the theoretical yield is 6.50 grams, and the percent yield is 100%.