Loss Electrons →Oxidation →Reducing Agent
Gain Electrons →Reduction →Oxidizing Agent
2 N2H4 + N2O4 → 3 N2 + 4 H2O
Step 2: Oxidation states
H (connected to nonmetal) = +1
2(N) + 4(+1) = 0
2(N) + (+4) = 0
2(N) = - 4
N = - 4/2
N = - 2
O (peroxide) = -1
2(N) + 4(-1) = 0
2(N) + (-4) = +4
N = + 4/2
N = + 2
What is being oxidized, and what is being reduced? Which substance serves as the reducing agent, and which as the oxidizing agent?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Redox Reactions concept. If you need more Redox Reactions practice, you can also practice Redox Reactions practice problems.
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Based on our data, we think this problem is relevant for Professor Bindell's class at UCF.