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The above graph depicts solubility in water at various temps. If we are dissolving in polar water, why is methane more soluble than a polar molecule like carbon monoxide?

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    $\begingroup$ So, given the strong dependence on temperature, this implies that the solubility is driven more by entropic considerations than enthalpic considerations, as the latter should be relatively constant over different temperatures. That means that your question may be flawed in that polarity is not the driving factor of solubility for gases. $\endgroup$ – Zhe Feb 21 at 19:32
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    $\begingroup$ Carbon monoxide is much less polar than it might seem. $\endgroup$ – Ivan Neretin Feb 21 at 19:38
  • $\begingroup$ If CO were nonpolar wouldn't it experience greater dispersion forces due to its higher mass relative to methane? My book states that gas solubility should increase with mass. $\endgroup$ – gerry Feb 21 at 19:48
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    $\begingroup$ Well, it's molar solubility so value is already divided by molar mass... Weight percent for CO is higher then for CH4. $\endgroup$ – Mithoron Feb 21 at 21:11
  • $\begingroup$ Polarity get trumped by hydrogen bonds? $\endgroup$ – Charlie Crown Feb 22 at 5:32

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