Asked by cassie
2. What is the reduction half-reaction for the following unbalanced redox equation?
Cr2O7^2– + NH4^+ Cr2O3 + N2
A.) Cr2O3 -> Cr2O7^2–
B.) Cr2O7^2– -> Cr2O3
C.) NH4^+ -> N2
D.) N2 -> NH4^+
I think it is B...?
3. Which oxidation-reduction reactions are best balanced by the half-reaction method?
A.) covalent reactions
B.) acid-base reactions
C.) ionic reactions
D.) intermolecular reactions
I think it is C....?
Cr2O7^2– + NH4^+ Cr2O3 + N2
A.) Cr2O3 -> Cr2O7^2–
B.) Cr2O7^2– -> Cr2O3
C.) NH4^+ -> N2
D.) N2 -> NH4^+
I think it is B...?
3. Which oxidation-reduction reactions are best balanced by the half-reaction method?
A.) covalent reactions
B.) acid-base reactions
C.) ionic reactions
D.) intermolecular reactions
I think it is C....?
Answers
Answered by
DrBob222
With practice you will learn what oxidizes and what reduces. To help let me give you the oxidation states and you figures these out for yourself.
Cr is +6 on the left and +3 on the right.
N is -3 on the left and zero on the right.
For the second question, AFTER you have balanced the reactions as far as change of electrons is concerned, don't you usually add H^+ (if acid) or OH^-(if base) and water? So what's the answer.
Cr is +6 on the left and +3 on the right.
N is -3 on the left and zero on the right.
For the second question, AFTER you have balanced the reactions as far as change of electrons is concerned, don't you usually add H^+ (if acid) or OH^-(if base) and water? So what's the answer.
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