How do we represent the oxidation of a #31.7*g# mass of iron by chlorine gas? What mass of #FeCl_3(s)# results?

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How do we represent the oxidation of a #31.7*g# mass of iron by chlorine gas? What mass of #FeCl_3(s)# results?

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Answer 1 · 2015-11-03T20:38:48

#Fe(s) + 3/2Cl_2(g) rarr FeCl_3(s)#

Explanation:

Moles of iron: #(31.7*g)/(55.85* g* mol^-1)# #=# #??*mol#

This molar quantity of iron requires #3/2# molar equivalents of chlorine gas for complete reaction. What is oxidized, and what is reduced in the reaction? How do you know?

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How do we represent the oxidation of a #31.7*g# mass of iron by chlorine gas? What mass of #FeCl_3(s)# results?

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