The information below describes a redox reaction. cr3+(aq)+2cl-(> cr(s)+cl2(s) 2cl-(> cl2(g)+2e- cr3+(aq)+3e- > cr(s) what is the final, balanced equation for this reaction? 1.) 2cr3+(aq)+6cl-(aq) > 2cr(s)+3cl2(g) 2.) 2cr3(aq)+2cl-(aq)+6e- > cl2(g)+2cr(s) 3.) cr3+(aq)+6cl-(aq)+3e- > 2cr(g)+3cl2(g) 4.) cr3+(aq)+2cl-(> cr(s)+cl2(g)

option 1)  2Cr3+(aq)+6Cl-(aq) ------> 2Cr(s)+3Cl2(g)

Explanation:

1) Write the oxidation half-reaction:



2) Write the reduction half-raction:



3) Multiply each half-reaction by the appropiate coefficient to equal the number of electrons of both half-reactions.



4) Add both half-reactions



And that is the answer. You can count the atoms and charges on every side and check they are equal.

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Idont really know sorry