When 2 g of gaseous substance a are introduced into an initially evacuated flask kept at 25°c, the pressure is found to be 1 atm. three grams of gaseous substance b are then added to the 2g of a, and the pressure is now found to be 1.5 atm. assuming ideal gas behavior. calculating the ratio of molecular weights, that is, mwa /mwb

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Explanation:

From the ideal gases law we have:

P= pressure, V= volume of the container, n= mol of gas, R=constant of gases and T=temperature.

The molecular weight is:

m is mass.

The dalton's law tell us that the total pressure of a mixture of gases is the sum of the partial pressure of every gas.

the relationship between the molecular weights is:

(equation 1)

where

Replacing in equation 1

since V and T are constante

we don't know the partial pressure of B but we know the partial pressure of A since it was the pressure of A at the beginning before adding B (1 atm). We also also know the total pressure of the container with both gases (1.5 atm). From the dalton's law

now

a  solution  is always transparent, light passes through with no scattering from solute particles which are molecule in size. the  solution  is homogeneous and does not settle out. a colloid is intermediate between asolution  and a  suspension. while asuspension  will separate out a colloid will not.

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.