Question

at constant temperature, the pressure of carbon dioxide over water increases from 1:00 atm to 3:00 atm. if the beginning solubility is 0.878g/100 L water, what is the final solubility

Answer 1

Answer:

Calculate the solubility of carbon dioxide in water at 0 °C and a pressure of 3.00 atm. The solubility of carbon dioxide is 0.348 g/100 mL ...

Answer 2

Answer:

Explanation:

Concept:

The solubility, which depends on gas pressure, is a measurement of the concentration of dissolved gas particles in the liquid. A gas's solubility increases with higher pressure while falling with lower pressure because of an increase in collision frequency.

Given:

The initial pressure$(P_{1} )$ is $1.00$ atm.

The Final pressure$(P_{2} )$ is $3.00$ atm.

The initial solubility $(S_{1} )$ is $0.878g/100 L$ water.

Find:

To find the final solubility of water.

Solution:

According to Henry's law we know that solubility is directly proportional to pressure of gas.

So that,

$\frac{P_{1} }{P_{2}} =\frac{S_{1} }{S_{2}} \\\frac{1.00 atm}{3.00 atm} =\frac{0.878g/100 L water}{S_{2} } \\S_{2}=\frac{(3.00) (0.878g/100 L water) }{1.00}\\ S_{2}= 2.63 g/100 L water$

Therefore, the required final solubility of water is $2.63g/100 L$ water.

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