A mixture of two gases with a total pressure of 2.00 atm contains 0.70 atm of Gas A. What is the partial pressure of Gas B in atm?

The partial pressure of Gas B in the mixture of two gases has been 1.3 atm.

The partial pressure of the gas can be defined as the pressure of the particular gas in the mixture of gases.

According to dalton, the total pressure of the gas has been the sum of the partial pressure of the individual gases.

Thus, total pressure = partial pressure of gas A + partial pressure of gas B

Given, total pressure = 2 atm

The partial pressure of gas A = 0.70 atm

So, the partial pressure of Gas B = total pressure - partial pressure of gas A

The partial pressure of Gas B = 2.0 atm - 0.70 atm

The partial pressure of Gas B = 1.3 atm

Thus, the partial pressure of Gas B in the mixture of two gases has been 1.3 atm.

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The partial pressure of Gas B : 1.3 atm

Dalton's Law stated

the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases  

Can be formulated:  

P tot = 2 atm

P gas A = 0.7 atm

So P gas B :

fe 55.85 g/mol and h2o 18.02 g/mol.