Answer:
The total pressure exerted by mixture of gas is equal to the sum of the partial pressure of individual 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
Answer:contact forces or transfer energy(not sure)
Explanation:
An elephant. It's not wrong.
Answer:
all of the above I'm pretty sure
Answer : The vapor pressure of the dry oxygen gas is, 736.2 torr
Explanation : Given,
Volume of sample of oxygen = 500 mL
Vapor pressure of oxygen + water = 760 torr
Vapor pressure of water = 23.8 torr
Now we have to determine the vapor pressure of the dry oxygen gas.
Vapor pressure of the dry oxygen gas = Vapor pressure of (oxygen + water) - Vapor pressure of water
Vapor pressure of the dry oxygen gas = 760 torr - 23.8 torr
Vapor pressure of the dry oxygen gas = 736.2 torr
Thus, the vapor pressure of the dry oxygen gas is, 736.2 torr