Answers

2015-04-26T02:09:39+05:30

This Is a Certified Answer

×
Certified answers contain reliable, trustworthy information vouched for by a hand-picked team of experts. Brainly has millions of high quality answers, all of them carefully moderated by our most trusted community members, but certified answers are the finest of the finest.
Henry's law:

.\ \ \ partial\ pressure\ p=k_H\ c,\\. \ \ \ \ \ \ where\ c=concentration\ of\ gas\ in\ solution,\\.\ \ \ \ \ \ k_H=Henry's\ constant

k_H=1.67*10^8\ Pa\ at\ 298\ {}^0 K\\p=2.5\ atm=2.5*1.013*10^5\ Pa\\\\c=\frac{p}{k_H}=\frac{2.5*1.013*10^5}{1.67*10^8}=1.516*10^{-3}\ \frac{moles}{Litre}\\\\mass=c*volume\ of\ solution=1.516*10^{-3}\ \frac{mole}{Litre}*\frac{500}{1000}litre

Molecular mass of carbon dioxide = 12+2*16=44

Mass of CO₂ dissolving in 500 ml of water at a pressure of 2.5 atm at 298 °K =
            44 * 0.758 * 10⁻³ = 33.352 mg.


1 5 1
  • Brainly User
2015-04-26T20:14:55+05:30
Henry's law:





Molecular mass of carbon dioxide = 12+2*16=44

Mass of CO₂ dissolving in 500 ml of water at a pressure of 2.5 atm at 298 °K =
            44 * 0.758 * 10⁻³ = 33.352 mg.
0