Question #992b4

1 Answer
anor277
Dec 22, 2016

It looks like that the sulfate has the greater molar quantity of the sulfur. We have to find the #"molar quantity............"#

Explanation:

And to find #"molar quantity"#, we take the quotient, #"Mass (g)"/("Molar mass (g"*mol^-1")"#, and get an answer with units #1/(mol^-1)=1/(1/(mol))=mol# as required.............

#"Moles of thiocyanate"# #=# #(13.4*g)/(97.18*g*mol^-1)=??*mol#

#"Moles of aluminum sulfate"# #=# #0.067*mol#

Because potassium thiocyanate has a formula of #KSCN#, and aluminum sulfate has a formula of #Al_2(SO_4)_3#, clearly there are more sulfur atoms in the sulfate, i.e. #3xx0.067*mol# versus #0.138*mol#. Claro?

Related questions
See all questions in The Mole
Impact of this question
1746 views around the world
You can reuse this answer
Creative Commons License