What is the theoretical volume (at STP) of butene product that can be obtained
from the dehydration of 0.412 g of 2-butanol? (MW = 74 g/mol; 22.414 L/mol)
A. 125 L
B. 1.36 L
C. 125 mL
D. 0.000248 L
Can you please show calculations
Show you thinking and we will comment. We don't do the homework for you.
I thought that it would be 125 ml...I don't thing it is write though... I think I did the conversation wrong though... All I want to know is how to do the conversation correctly..
To calculate the theoretical volume of butene product, we need to convert the given mass of 2-butanol to moles, then use the stoichiometry of the reaction to determine the moles of butene produced, and finally convert those moles to volume using the molar volume at standard temperature and pressure (STP).
First, let's calculate the moles of 2-butanol:
Given mass of 2-butanol = 0.412 g
Molar mass of 2-butanol (MW) = 74 g/mol
Moles of 2-butanol = 0.412 g / 74 g/mol
Moles of 2-butanol = 0.00557 mol
Next, we need to use the balanced chemical equation for the dehydration of 2-butanol to determine the stoichiometry and find out the moles of butene produced. The equation is:
2-butanol -> butene + H2O
From the equation, we see that 1 mole of 2-butanol produces 1 mole of butene.
Therefore, moles of butene produced = 0.00557 mol
Finally, we can calculate the volume of butene at STP using the molar volume:
Molar volume at STP = 22.414 L/mol
Volume of butene = moles of butene * molar volume at STP
Volume of butene = 0.00557 mol * 22.414 L/mol
Volume of butene = 0.1247 L
Thus, the correct answer is C. 125 mL, which is equivalent to 0.125 L.