I need serious help on this....please help guys.. i've to turn it in in an hours...
Balance th following equation in acid Solutiong and determind if it is spontaneous under standard conditions.
NO3^-1 + Sn^+2 ---> NO + Sn^+4
Please do not post duplicates.
To balance the equation in acid solution, follow these steps:
Step 1: Write down the unbalanced equation.
NO3^-1 + Sn^+2 ---> NO + Sn^+4
Step 2: Balance the non-hydrogen and non-oxygen atoms first.
There are no nitrogen (N) atoms on the right side of the equation, so we need to add a coefficient of 2 in front of NO.
2NO3^-1 + Sn^+2 ---> 2NO + Sn^+4
Now, let's balance the tin (Sn) atoms. On the left side, we have one tin atom (Sn^+2), and on the right side, we have one tin atom in Sn^+4. So, the tin atoms are already balanced.
Step 3: Balance the oxygen atoms.
On the left side, we have six oxygen atoms from the two NO3^-1 ions, and on the right side, we have two oxygen atoms from NO. To balance the oxygen, add a coefficient of three in front of NO.
2NO3^-1 + Sn^+2 ---> 3NO + Sn^+4
Step 4: Balance the charge.
On the left side, we have a total charge of -2 from the two NO3^-1 ions. On the right side, the Sn^+4 ion has a charge of +4, and the three NO molecules are neutral. To balance the charge, add a coefficient of 2 in front of Sn^+2 and a coefficient of six in front of NO.
2NO3^-1 + 2Sn^+2 ---> 3NO + Sn^+4
Now, the equation is balanced in acid solution.
To determine if the reaction is spontaneous under standard conditions, we need to calculate the standard cell potential (E°). The standard potential of the overall cell can be determined by the standard potentials of the individual half-reactions.
For the given equation, it involves a redox reaction between Sn^2+ and Sn^4+. You can look up the standard reduction potentials for these species. Since the reaction involves Sn^2+ gaining two electrons to form Sn^4+, the half-reaction is:
Sn^2+ + 2e^- -> Sn^4+ with standard potential E°(Sn^4+ / Sn^2+).
If E°(Sn^4+ / Sn^2+) is positive, then the reaction is spontaneous under standard conditions. If it is negative, the reaction is not spontaneous. You can refer to a standard reduction potential table to find the value and determine if the reaction is spontaneous.
Remember to double-check the balanced equation and don't include duplicate posts. Good luck!