Question

After the completion of a gas forming reaction, the column of water remaining in the collection flask was measured to me 55 mm high, the vapor pressure of water is 0.0313 atm at 25oC, and the atmospheric pressure that day was measured as 0.950 atm, what is the partial pressure of the gas produced by the reaction

Answer 1

The partial pressure of the gas produced by the reaction is 0.9187 atm

Step-by-step explanation:

Given;

vapor pressure of water,
`\rho_w` = 0.0313 atm

measured atmospheric pressure,
`P_(Total)` = 0.950 atm

partial pressure of the gas produced by the reaction = ?

According to Dalton's law of partial pressure; total pressure is equal to sum of partial pressure of water vapor and gas produced.

`P_(Total) = P_(gas) + P_(water)`

`P_(gas)` =
`P_(Total) -P_(water)`

`P_(gas)` = 0.95 - 0.0313

`P_(gas)` = 0.9187 atm

Therefore, the partial pressure of the gas produced by the reaction is 0.9187 atm