Answer to Question #185868 in General Chemistry for Catherine

Question

If 10.0 mL of 2.50 M SrS (aq) is made to react with 25.0 mL of 1.50 M ZnSO4 (aq), how many moles of the excess reactant will be left after the reaction? Express your answer in three significant figures.

Answer 1

ZnSO₄+SrCl₂ $\implies$ ZnCl₂+SrSO₄

ZnSO₄+SrS$\implies$ ZnS+SrSO₄

But SrS_(aq)=Volume (10mL)

M(2.50M)

$Moles=\frac{V×M}{1000}$

$=\frac{10×2.5}{1000}$ $=0.025moles$

ZnSO_4(aq)=$\frac{V×M}{1000}$

=$\frac{25×1.5}{1000}=0.0375moles$

Therfore:

Moles of ZnS using mole ratio=$0.0375moles$

Moles of SrSO₄ using mole ratio =

$0.025moles$

Excess reactants ZnSO₄ moles produced=$(0.0375-0.025)moles$

$=0.0125moles$