🤓 Based on our data, we think this question is relevant for Professor Medina's class at MDC.
We are asked to determine the molecular formula of a compound with a molar mass of 180.18 g/mol and a percentage composition of 39.99% C, 6.73% H, 53.28% O.
This means we need to do the following steps:
Step 1: Calculate the mass and moles of C, H, and O in the compound.
Step 2: Determine the lowest whole number ratio of C, H, and O to get the empirical formula.
Step 3: Get the ratio of the molar mass and empirical mass to determine the molecular formula.
Step 1: The compound is composed of C, H, O and we’re given the mass percent of C (39.99% C), H (6.73% H) and O (53.28% O). Check if the mass percentages of a compound add up to 100%.
Recall that mass percent is given by:
Assuming we have 100 g of the compound, this means we have 39.99 g C, 6.73 g H, and 53.28 g O.
Now, we need to get the moles of each element in the compound.
The atomic masses are 12.01 g/mol C, 1.00 g/mol H, 15.99 g/mol O.
A compound has a molar mass of 180.18 g/mol. Given the following percent composition, calculate the molecular formula.
39.99% C, 6.73% H, 53.28% O