Balance the following redox equation by the oxidation number methode
Ag + HNO3 = AgNO3 + NO + H2O
http://www.chemteam.info/Redox/Redox.html
Ag changes from zero to +1. N (in HNO3) changes from +5 to +2(in NO). Note that some of the NO3^- ions don't change at all.
i have all the oxidation numbers for all the of elements but i don't understand how i'm supposed to balance the equation using the oxidation numbers.
Do i have to to change the oxidation numbers to equation the same on each side?
To balance the given redox equation using the oxidation number method, you need to follow these steps:
Step 1: Assign oxidation numbers to all the elements in the reactants and products.
Ag + HNO3 = AgNO3 + NO + H2O
The oxidation number of Ag is +1 in Ag (since it is a Group 11 metal) and +1 in AgNO3 (AgNO3 is a neutral compound). The oxidation number of N in HNO3 is +5 (since it is in Group 15 and is bonded with three oxygen atoms) and +2 in NO (nitric oxide). The oxidation number of H is +1 throughout the equation, and O is -2 in HNO3 and AgNO3, while it is 0 in NO and -2 in H2O.
Step 2: Identify the elements that are undergoing oxidation and reduction.
In this equation, Ag is being reduced from +1 to 0, and N is being oxidized from +5 to +2.
Step 3: Balance the atoms and charges using coefficients.
First, let's balance the atoms, starting with Ag and N:
Ag + HNO3 => AgNO3 + NO
Counting the number of Ag atoms, we have 1 Ag on the left side and 1 Ag on the right side.
Next, focus on nitrogen (N) atoms. We have 1 N on the left side (in HNO3) and 1 N on the right side (in AgNO3 and NO).
Now, let's balance oxygen (O) atoms. On the left side, there are 3 O atoms in HNO3, so we need 3 O atoms on the right side. We can achieve this by adding a coefficient of 3 to H2O on the right side:
Ag + HNO3 => AgNO3 + NO + 3H2O
At this point, the atoms are balanced, but charges are not. To balance the charges, we need to add electrons (e-) to the equation:
Ag + HNO3 => AgNO3 + NO + 3H2O + e-
To balance the charges, we need to know the overall charge of the reaction. Since there are no other indications, we assume it is neutral. Considering that AgNO3 is a neutral compound, the total charge of Ag must be +3 to balance the overall equation. Therefore, we need to add 3 electrons to the left side:
Ag + 3e- + HNO3 => AgNO3 + NO + 3H2O + e-
Now, we have balanced both atoms and charges.
Step 4: Make sure the electrons are balanced.
In this equation, the electrons needed on the left side (3e-) and the electrons produced on the right side (e-) do not cancel each other out. To balance the electrons, we need to multiply the whole equation by 3:
3Ag + 9e- + 3HNO3 => 3AgNO3 + 3NO + 9H2O + 3e-
Now, we can simplify the equation:
3Ag + 3HNO3 => 3AgNO3 + 3NO + 9H2O
As a result, the balanced chemical equation using the oxidation number method is:
3Ag + 3HNO3 => 3AgNO3 + 3NO + 9H2O