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# chemistry question involving Henry's law and solubility of gases in liquids?

How many liters of carbon

dioxide, reduced to standard conditions of

temperature and pressure (25 °C and 1 atm, respectively), will dissolve in 1 liter of water at 25 °C when the partial pressure of gas is 0.7 atm?

These may be useful, though I am not sure how to solve the question.

Henry's law is P =k(h) * x

and k(h) = 1.64 * 10^3 atm/mole fraction

Mw of CO2 = 44g/mol.

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Henry’s Law: At constant temperature, he amount of dissolved gas in a volume of a specified liquid id directly proportional to the partial pressure of the gas above the liquid.

Pressure = Henry’s Law constant x concentration

P = KH*C units of KH = atm/mole fraction

0.70 atm = 1.64 x 10^3 atm/mole fraction* C

C = 0.7 atm / 1.64 x 10^3 atm/ mole fraction

Mole Fraction = 4.27 x 10^-4

Moles CO2 / moles H2O + moles CO2 = mole fraction

1.0 liter of water = 1000 g x 1 mole H2O = 55.6 moles H2O

Let y = moles CO2

y/ y + 55.6 moles H2O = 4.27 x 10^-4

y = 4.17 x 10^-4y + 0.0237

0.9995 = 0.0237

y = 0.0232 moles CO2/liter

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