Question

193ml of O2 was collected over water on a day when the atmospheric pressure was 762.0mm Hg, the temperature of water was 23.0°C, and vapor pressure was 21.1. What is the partial pressure of O2 collected?

Options:
a. 148.8 mm Hg
b. 174.9 mm Hg
c. 190.9 mm Hg
d. 205.0 mm Hg

Answer 1

The partial pressure of O2 is found by subtracting the vapor pressure of water (21.1 mm Hg) from the atmospheric pressure (762.0 mm Hg), which results in a value of 740.9 mm Hg. This value does not match any of the provided options, but option (c) is the closest.

Step-by-step explanation:

To determine the partial pressure of O2 collected over water, you subtract the vapor pressure of water from the total atmospheric pressure. In this case, the atmospheric pressure is 762.0 mm Hg, and the vapor pressure of water at 23.0°C is 21.1 mm Hg.

So, the calculation would be:

Partial Pressure of O2 = Atmospheric Pressure - Vapor Pressure of Water

= 762.0 mm Hg - 21.1 mm Hg

= 740.9 mm Hg

Therefore, the correct option that represents the partial pressure of O2 is slightly different from those provided. As the subject expert, I've provided the accurate calculation, which shows none of the given options are correct. However, option (c) is the closest to the accurate value.