How many grams of the molecule in the figure above would be required to make 1 L of a 0.5 M solution of the molecule?
H O
| || (looks like C=O on the vertical)
H-C-C-O-H
|
H
a.29
b.30
c.60
d.150
e.342
30
To find out how many grams of the molecule are required to make a 0.5 M solution in 1 L, we need to follow these steps:
Step 1: Calculate the molar mass of the molecule.
Looking at the structure of the molecule, we can see that it is composed of 4 hydrogen atoms (H), 1 carbon atom (C), and 1 oxygen atom (O). The molar mass of hydrogen is approximately 1 g/mol, carbon is 12 g/mol, and oxygen is 16 g/mol.
So, the molar mass of the molecule is:
(4 * 1 g/mol) + (1 * 12 g/mol) + (1 * 16 g/mol) = 4 + 12 + 16 = 32 g/mol
Step 2: Calculate the moles of the molecule required to make a 0.5 M solution in 1 L.
The molarity (M) of a solution is defined as moles of solute per liter of solution. In this case, the molarity is 0.5 M, and we want to make 1 liter of the solution.
So, the moles of the molecule required can be calculated as:
moles = molarity * volume
moles = 0.5 M * 1 L = 0.5 mol
Step 3: Convert moles to grams.
To convert moles to grams, we can use the molar mass of the molecule calculated in Step 1.
grams = moles * molar mass
grams = 0.5 mol * 32 g/mol = 16 g.
Therefore, to make a 0.5 M solution of the molecule in 1 L, we would require 16 grams of the molecule.
None of the answer choices provided matches this result, so it seems there might be a discrepancy between the given structure and the molar mass calculation.