For the equation Ag + NO3 - à Ag + + NO?

Question

Step 1: What substance is reduced?

Step 2: What substance is oxidized?

Step 3: What is the half reaction for oxidation?

Step 4: What is the half reaction for reduction?

Step 5: What is the net balanced equation?
Step 6: What is the reduced equation?




2. When first learning to balance equations, we learned that the number of atoms of each element in the products and reactants must be equivalent. What are some additional factors that must be taken into account when balancing equations for redox reactions?

3. What are half reactions?

4. What two aspects of the half-reaction equations must be balanced?

Answer 1

OILRIG
3Ag(s) + 4HNO3(aq) → 3AgNO3(aq) + 2H2O(l) + NO(g)

(1) Reduction is gain (of electrons)

NO3 gains electron(s) and is therefore reduced

(2) Oxidation is loss (of electrons)

Ag loses electron(s) and therefore is oxidized

(3) Ag -> Ag+ + e-

(4) 4NO3- + 3e- -> 3NO3- + 2O-- + NO

(5) 3Ag(s) + 4NO3-(aq) + 4H+ → 3AgNO3(aq) + 2H2O(l) + NO(g)

(6) ??
unless I've done this in (5) and 5 is supposed to be (2)X3 to give off the 3e-

Q2 In addition to balancing atoms of each element, it is important to balance numbers of electrons gained and lost in the REDOX

Q3 Half reactions are the interactions between the ion/molecule and the electrons. One of the half-reactions describes loss of electrons (oxidation) - step 3, above - and the other of the half-reactions describes gain of electrons (reduction) - step 4 above

Q4 Balance the numbers of atoms of each element before and after. Balance the charge of the ions on each side. (Also balance the number of electrons lost by the reducing agent with the number of electrons gained by the oxidising agent. This should be accounted for by balancing the charge.)

Answer 2

Check your textbook! its in there!