Step 1

$\mathbf{5}\mathbf{.}\mathbf{76}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{Ag}}_{\mathbf{2}}\mathbf{O}}\mathbf{}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{Ag}}_{\mathbf{2}}\mathbf{O}}}{\mathbf{231}\mathbf{.}\mathbf{735}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{Ag}}_{\mathbf{2}}\mathbf{O}}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\mathbf{mol}\mathbf{}{\mathbf{O}}_{\mathbf{2}}}{\mathbf{2}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{Ag}}_{\mathbf{2}}\mathbf{O}}}$** = 0.01243 mol O _{2}**

Silver oxide decomposes when heated:

2 Ag_{2}O(s) → 4 Ag(s) + O_{2}(g)

If 5.76 g of Ag_{2}O is heated and the O_{2} gas produced by the reaction is collected in an evacuated flask,what is the pressure of the O_{2} gas if the volume of the flask is 0.65 L and the gas temperature is 25 ^{o}C?

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