Balance the following reaction A coefficient of "1"is understood. Choose option "blank" for the correct answer if the coefficient is "1." div PbO_(2)arrow PbO+ AO_(2)

To balance the given chemical reaction, we need to ensure that the number of atoms of each element is the same on both sides of the equation.The unbalanced reaction is: Let's identify the elements involved: Pb (lead) and O (oxygen).1. **Balance Lead (Pb):** There is 1 Pb atom on both sides of the equation, so lead is already balanced.2. **Balance Oxygen (O):** On the left side, there are 2 oxygen atoms in . On the right side, there is 1 oxygen atom in and 2 oxygen atoms in , totaling 3 oxygen atoms.To balance the oxygen atoms, we can adjust the coefficients:- Multiply by 2 to have 2 oxygen atoms from and 2 from , totaling 4 oxygen atoms on the right side.Now the balanced equation looks like this: However, this doesn't match the original format with "AO_2". Assuming "A" was a placeholder for balancing purposes, let's correct it: Since fractional coefficients are not typically used in balanced equations, multiply the entire equation by 2 to eliminate the fraction: Thus, the balanced equation is: In terms of coefficients, the answer is:- For : 2- For : 2- For : 1If you need to choose options based on these coefficients, they would be:- : 2- : 2- : blank (since the coefficient is 1)