Question

A sample of oxygen collected over water at a temperature of 29.0 °C and a pressure of 764 torr has a volume of 0.560 L. What volume would the dry oxygen have under the same conditions of temperature and pressure?

Answer 1

To find the volume of dry oxygen under the same conditions, subtract the vapor pressure of water from the total pressure and use the combined gas law equation. The volume of dry oxygen would be approximately 0.539 L.

Step-by-step explanation:

To find the volume of dry oxygen under the same conditions of temperature and pressure, we need to account for the vapor pressure of water at 29.0 °C. The vapor pressure of water at this temperature is 30.0 torr. This means that the partial pressure of oxygen is 764 torr - 30 torr = 734 torr.

Using the combined gas law, we can set up the following equation: P1V1/T1 = P2V2/T2

Since we're keeping the temperature and pressure constant, we can rearrange the equation to solve for V2:

V2 = (P1 * V1) / P2

Plugging in the values, we have:

V2 = (734 torr * 0.560 L) / 764 torr = 0.539 L