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The formula that governs the concentration of gas dissolved in a solvent based on its pressure is given by Henry's Law C kP Where: C solubility of a gas at a fixed temperature (in mol/L, M) k Henry's Law constant (in units of mol/L atm) P partial pressure of the gas (in units of atm).How many grams of carbon dioxide gas is dissolved in a 265 mL can of cola if the manufacturer uses a pressure of 1.7 atm in the bottling process at 25 °C? Assume that the k of CO2 in water = 0.034 mol/L·atm) at 25 °C. Report your answer to two significant figures.

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dsdrajlin

Answer:

0.68 g

Explanation:

The solubility of a gas (C) in a liquid can be calculated from Henry's law.

C = k . P

where,

k: Henry's Law constant

P: partial pressure of the gas

C = (0.034 mol/L.atm) . 1.7 atm = 0.058 mol/L

The molar mass of CO₂ is 44.01 g/mol. The mass of CO₂ in 265 mL (0.265 L) of solution is:

[tex]0.265L.\frac{0.058mol}{L} .\frac{44.01g}{mol} =0.68g[/tex]

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