Chemistry, 21.10.2020 16:01 thedaisylopez3628
Assume that silver and gold form ideal, random mixtures. Calculate the mass of pure Ag needed to cause an entropy increase of 20 J/K when mixed with 100g of pure Au
Answers: 3
![\Delta S=-n_TR\Sigma[x_i*ln(x_i)]](/tpl/images/0827/7699/ef17c.png)
![\Delta S=-(n_{Au}+n_{Ag})R\Sigma[\frac{n_{Au}}{n_{Au}+n_{Ag}} *ln(\frac{n_{Au}}{n_{Au}+n_{Ag}} )+\frac{n_{Ag}}{n_{Au}+n_{Ag}} *ln(\frac{n_{Ag}}{n_{Au}+n_{Ag}} )]](/tpl/images/0827/7699/1af49.png)
representing the moles of silver:![20\frac{J}{mol}=-(0.508+x)8.314\frac{J}{mol*K} \Sigma[\frac{0.508}{0.508+x} *ln(\frac{0.508}{0.508+x} )+\frac{x}{0.508+x} *ln(\frac{x}{0.508+x} )]](/tpl/images/0827/7699/365c1.png)
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Assume that silver and gold form ideal, random mixtures. Calculate the mass of pure Ag needed to cau...
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