Question #ca9c5

1 Answer
anor277
May 24, 2016

Approx. #103*g#

Explanation:

#"Moles of copper"# #=# #(82*g)/(63.55*g*mol^-1# #=# #1.29*mol#.

#"Moles of sulfur"# #=# #(25*g)/(32.06*g*mol^-1# #=# #0.78*mol#.

Clearly the sulfur oxidant is in excess if the copper is incompletely oxidized; #0.66*mol# #Cu_2S# may be formed,

#0.66*molxx159.16*g*mol^-1# #=# #??g#

Look at your stoichiometric equation and divide by 2.

#2Cu + S rarr Cu_2S#

It tells you that approx. #63*g# of copper metal react with approx. #16*g# of sulfur. Why? Because that is the molar mass of each element is #63.55*g# and #32.06*g# respectively. Good luck in your test.

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