Question

a compound is found to have the empirical formula ch₂o and a molar mass of 180.0 g/mol. what is the molecular formula of this compound? please enter your answers as numerical digits (i.e. 9). if any of your answers are 1, please write this even though the number 1 is generally assumed in chemical formulas.

question 9
5 pts
for the bunsen burner, if the flame is yellow, then this means _______.
not enough gas
too much oxygen
too much gas
not enough oxygen

Explanation:

Step1: Calculate empirical - formula mass

The atomic masses of C = 12.01 g/mol, H = 1.01 g/mol, and O = 16.00 g/mol. For the empirical formula \(CH_2O\), the empirical - formula mass \(M_{empirical}=(1\times12.01)+(2\times1.01)+(1\times16.00)=30.03\ g/mol\).

Step2: Determine the multiple \(n\)

We know that the molar mass of the compound \(M = 180.0\ g/mol\). The multiple \(n=\frac{M}{M_{empirical}}=\frac{180.0}{30.03}\approx6\).

Step3: Find the molecular formula

Multiply the sub - scripts in the empirical formula by \(n\). The molecular formula is \(C_{1\times6}H_{2\times6}O_{1\times6}=C_6H_{12}O_6\).

For the Bunsen burner question:
A yellow flame in a Bunsen burner indicates that there is not enough oxygen for complete combustion.

Answer:

For the first part:
C: 6
H: 12
O: 6
For the second part: not enough oxygen