Which best defines partial pressure in a mixture of gases?
o pressure that is exerted by all the gases of a mixture on the container
o pressure that is exerted by one gas as if it occupied a container by itself
o half of the pressure that is exerted by the gases of a mixture on the container
sum of the individual pressures that are exerted by two or more gases

sum of the individual pressures that are exerted by two or more gases

Explanation:

According to Dalton law of partial pressure,

The total pressure exerted by mixture of gas is equal to the sum of the partial pressure of individual gases.

Mathematical expression:

P(total) = P₁ + P₂ + P(n)

P₁= Partial pressure of one gas

P₂ = Partial pressure of second gas

Pn = Partial pressure of number of gases

For example:

A gaseous mixture consist of He and Ne gas . The pressure exerted by He is 2 atm while neon exerted 4 atm. The total pressure will be:

P(total) = P(He) + P(Ne)

P(total) = 2 atm + 4 atm

P(total) =  6 atm

sum of the individual pressures that are exerted by two or more gases

Explanation:

the mass of the cathode increases because ions from the solution get reduced to atoms and become part of the cathode.

explanation:

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