would the molar mass of a volatile liquid, calculated using the procedure in this experiment, be incorrectly high, incorrectly low, or unaffected by the following?

You forgot to measure the volume of the flask, so you used the volume printed on the g=flask for your calculations.

and

Your unknown liquid had a boiling point of 102.3C.

any help would be much appreciated!

It would be nice to know what experiment you are discussing.

To determine whether the molar mass of the volatile liquid would be incorrectly high, incorrectly low, or unaffected in the given scenarios, we need to consider the effect of each scenario on the calculations.

1. Forgetting to measure the volume of the flask and using the printed volume on the flask for calculations:
By not accurately measuring the volume of the flask, you would introduce an error in the determination of the mass of the volatile liquid. The printed value may not accurately represent the true volume of the flask, leading to an incorrect determination of the mass. Since molar mass is calculated based on the mass of the substance and the volume it occupies, an inaccurate mass would affect the accuracy of the molar mass calculation. Therefore, this scenario would result in an incorrectly high or low molar mass, depending on whether the printed volume is greater or lesser than the actual volume of the flask.

2. The unknown liquid has a boiling point of 102.3°C:
The boiling point of a substance provides information about its volatility and the strength of intermolecular forces present. It does not directly affect the molar mass calculation. So, the boiling point of 102.3°C would not have any impact on the molar mass calculation.

In summary, the molar mass of the volatile liquid would only be affected by the first scenario, where an incorrect flask volume was used for calculations. The boiling point of the liquid, as given in the second scenario, would not affect the molar mass calculation.