Balance the following chemical equation. Drag the option from the list at the bottom to the correct spot. (4 points)

Question

(4 points)
Put responses in the correct input to answer the question. Select a response, navigate to the desired input and insert the response. Responses can be selected and inserted using the space bar, enter key, left mouse button or touchpad. Responses can also be moved by dragging with a mouse.
2Ag2O→
Response areaAg+
Response areaO2

0
4
6
8
6
2
10

Answer 1

To balance the chemical equation \(2 Ag_2O \rightarrow \) \(Ag + O_2\), we need to balance both silver (Ag) and oxygen (O) atoms.

1. On the left side, we have:

   • 4 Ag (from \(2 Ag_2O\)),
   • 2 O (from \(2 Ag_2O\)).

2. On the right side, if we have \(Ag\) and \(O_2\):

   • For \(O_2\), we have 2 O.

To balance the silver, we will need 4 silver atoms. For the silver, since each \(Ag_2O\) gives us 2 Ag, we need:

\[ 4 Ag \rightarrow 4 Ag \]

Thus, we match the Ag by making 4 Ag:

To write out the balanced equation, we need:

\[ 2Ag_2O \rightarrow 4Ag + O_2 \]

Inserting the appropriate responses into the blanks of the equation:

• For \(Ag\), we put 4 since that gives us 4 Ag atoms.
• For \(O_2\), we put 2 as we are producing 1 mole of \(O_2\), but we need it in the context of this final output.

Final balanced equation:

\[ 2Ag_2O \rightarrow 4Ag + \text{1 } O_2 \]

So, the balanced equation with the correct responses in the areas is:

Ag: 4
O2: 1