# Question #0462f

##### 1 Answer

#### Explanation:

You actually don't have enough information to solve this problem.

The idea here is that when a gas is collected over water, the **total pressure** of the sample will **include** the vapor pressure of water *at the temperature* at which the gas was collected.

SInce no mention of this vapor pressure was made, you will have to either look it up, or calculate it using the **Antoine equation**. But then again, you'd need to look up the Antoine constants for water, so I'll just use the known value without actually calculating it

http://www.endmemo.com/chem/vaporpressurewater.php

At

Now, according to **Dalton's Law of partial pressures**, the **total pressure** of a mixture of gases represents the **sum** of the partial pressures of each individual component of said mixture.

In your case, this can be written as

#P_"total" = P_"water" + P_"gas"#

This means that the pressure of the gas is equal to

#P_"gas" = P_"total" - P_"water"#

#P_"gas" = "751.5 mmHg" - "25.137 mmHg" = color(green)("726.4 mmHg")#