my tutor gave me this queston to practice with, but i've been working on it for over an hour and can't do it, could someone please guide me in the right direction? it's so confusing. I'm supposed to balance this equation using the oxidation states method:
KI + HNO3 ---> KNO3+ NO + I2 + H2O
KI + HNO3 ---> KNO3+ NO + I2 + H2O
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The I in KI has an oxidation number of -1 while on the other side the I2 has an oxidation number of 0. Therefore 2 electrons are lost per I2 molecule
The N in HNO3 has an oxidation number of +5, while the N in NO has an oxidation number of +2 therefore 3 electrons are gained by the N's
Multiply the K's on each side by 3 and make the HNO3 into 2HNO3 and the NO into 2NO. Now balance the I2 by putting a 3/2 in front of it. Then balance the H2O by putting a 2 in front of that. So the sequence of coefficients should be: 3, 4, 3, 1, 3/2, 2
To get rid of the 3/2 multiply everything by 2 YOu should now have 6, 8, 6, 2, 3, 4
The N in HNO3 has an oxidation number of +5, while the N in NO has an oxidation number of +2 therefore 3 electrons are gained by the N's
Multiply the K's on each side by 3 and make the HNO3 into 2HNO3 and the NO into 2NO. Now balance the I2 by putting a 3/2 in front of it. Then balance the H2O by putting a 2 in front of that. So the sequence of coefficients should be: 3, 4, 3, 1, 3/2, 2
To get rid of the 3/2 multiply everything by 2 YOu should now have 6, 8, 6, 2, 3, 4
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6KI + 8HNO3 = 6KNO3 + 2NO + 3I2 + 4H2O
in this reaction, I goes from I-1 to I neutral in I2, it loses an electron and is therefore oxidized. in turn, it is the reducing agent
N, in NO3-, is +5 and goes to N+2 in NO. it gains 3 electrons and is reduced. in turn, it is the oxidizing agent.
in this reaction, I goes from I-1 to I neutral in I2, it loses an electron and is therefore oxidized. in turn, it is the reducing agent
N, in NO3-, is +5 and goes to N+2 in NO. it gains 3 electrons and is reduced. in turn, it is the oxidizing agent.