The law of partial pressures or Dalton's law, formulated the British chemist John Dalton in 1802, establishes that <u>the pressure of a mixture of gases</u>, that do not react chemically, <u>is equal to the sum of the partial pressures that each of them would exert if only one occupied the entire volume of the mixture</u>, without changing the temperature.
In this way, <u>Dalton's law can be used to determine the total pressure in a container that has a mixture of gases</u>, each of which exerts a partial pressure, considering that all gases behave like ideal gases.
According to Dalton's law, the total pressure in the flask will be,

→ 
→ 
So, the total pressure in the flask is equal to 1.107 atm.