# Question 992b4

Dec 22, 2016

#### Answer:

It looks like that the sulfate has the greater molar quantity of the sulfur. We have to find the $\text{molar quantity............}$

#### Explanation:

And to find $\text{molar quantity}$, we take the quotient, $\text{Mass (g)"/("Molar mass (g"*mol^-1")}$, and get an answer with units $\frac{1}{m o {l}^{-} 1} = \frac{1}{\frac{1}{m o l}} = m o l$ as required.............

$\text{Moles of thiocyanate}$ $=$ (13.4*g)/(97.18*g*mol^-1)=??*mol#

$\text{Moles of aluminum sulfate}$ $=$ $0.067 \cdot m o l$

Because potassium thiocyanate has a formula of $K S C N$, and aluminum sulfate has a formula of $A {l}_{2} {\left(S {O}_{4}\right)}_{3}$, clearly there are more sulfur atoms in the sulfate, i.e. $3 \times 0.067 \cdot m o l$ versus $0.138 \cdot m o l$. Claro?