At $20$C$,$ the Henry$$s law constant, kH$,$ for O$2$ in water is $1\mathrm{.}34\backslash$times $108$ mol L$1$ Pa$1.$At $20C,$ the Henry's law constant, $k_H,$ for $O_2$ in water is $1\mathrm{.}34{10}^{-8}mol{L}^{-1}P{a}^{-1}.$

Calculate the mass of $O_2$ that would be dissolved per litre of water at atmospheric

pressure $(1\mathrm{.}013{10}^5(Pa))$ at this temperature.

Calculate the mass of O$2$ that would be dissolved per litre of water at atmospheric

pressure $(1\mathrm{.}013\backslash$times $105$ Pa$)$ at this temperature.