This question regards a lab using the ideal gas law to determine the molar volum

Question

This question regards a lab using the ideal gas law to determine the molar volume of oxygen. I'm confused on the part about equalizing pressures.

I ONLY need part 1B please. Please explain the problem and answer in detail, esp. what it has to do with equalization of pressure and how that works.

Here is the problem:

Here is the diagram:

And here is the procedure, just so you know what's going on:

Please let me know if you need anything else and thanks in advance!

1. Indicate how cach of the following errors would affect (increase, decrease, or no change) your calculated value for the molar volume of O, at STP assuming that you complete the experiment otherwise correctly). In e case, explain your After you finish heating your sample and the system cooled to room tem- perature, you closed the clamp on tube D without re-equalizing the pressures inside and outside of the flask. The water in beaker E was 4 inches deep and the water in flask C was 2 inches deep.

Explanation / Answer

Re-equalizing the pressure would mean that you make the pressure in both the containers C and E the same, most likely a value close to atmospheric pressure. Pressure increases with depth. Since the water in container E was 4 inch deep while that in container C was 2 inch deep, this would mean that the pressure of the gas in the container E was more than that in container C. Therefore, if the pressure is not equalized, then vapor will be sucked from the high pressure container (E) to the low pressure container; hence we need to re-equalize the pressure so that there is no pressure difference leading to flow of vapor/water in container C.

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