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How many grams of CO2 are dissolved in a 1.00 L bottle of carbonated water at 298 K if the pressure used in the carbonation process was 1.8 bar? The density of water at this temperature is 998 kg⋅m−3. The Henry's law constant for aqueous solution of CO2 at this temperature is 1.65×103bar.

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Answer:

[tex]0.048gCO_2[/tex]

Explanation:

Hello,

In this case, one uses the Henry's law to compute the carbon dioxide's concentration:

[tex]C_{CO_2}=\frac{1.8bar}{1.65x10^3bar/M}=1.09x10^{-3}M[/tex]

Now, by knowing the bottle's volume and carbon dioxide's molar mass,we obtain the grams as shown below:

[tex]m_{CO_2}=1.09x10^{-3}\frac{mol}{L}*\frac{44g}{1mol}*1.00L=0.048gCO_2[/tex]

Best regards.

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