Two beakers one containing 0.3 moles of NaCl dissolved in 4.5 moles of water, an

Question

Two beakers one containing 0.3 moles of NaCl dissolved in 4.5 moles of water, and the other containing 0.175moles NaCl dissolved in 0.6 moles of water, are placed inside of a sealed container. The container is kept at a constant Temperature T = 300k .The vapor pressure of pure water at this temperature is 3600 Pa. The two solutions in the container are left alone for a very long time until equilibrium is reached in the system .HINT: Water will be transferred from one beaker to another via vapor until the solutions in both beakers have the samevapor pressure. What are the final amounts (in moles) of water in each beaker after equilibrium is achieved? What is the partial pressure of the water in the container once equilibrium has been reached?

Explanation / Answer

let the number of moles transfered be n.so,

(4.5-n)/(4.5-n+0.3)=(0.6+n)/(0.6+n+0.175)

or n=1.279 mles

A)so the number of moles are 3.221 and 1.879.

B)partial pressure=3600*(3.221)/(3.221+0.3)

=3293.27 Pa

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