Balance the following reaction A coefficient of "I"is understood. Choose option "blank" for the correct answer if the coefficient is "1," :x+ : H_(2)Oarrow : N_(2)+ + xOH

To balance the chemical equation, we need to ensure that the number of each type of atom is the same on both sides of the equation. The given reaction is:<br /><br />\[ x + H_2O \rightarrow N_2 + xOH \]<br /><br />Let's assume "x" represents a compound containing nitrogen (N), and we need to balance it with water (H₂O) to produce nitrogen gas (N₂) and some hydroxide compound (xOH).<br /><br />1. **Balance Nitrogen (N):** <br /> On the right side, there are 2 nitrogen atoms in \( N_2 \). Therefore, we need 2 nitrogen atoms on the left side as well. This implies that there should be 2 molecules of the compound "x" if it contains one nitrogen atom per molecule.<br /><br />2. **Balance Hydrogen (H):** <br /> There are 2 hydrogen atoms in \( H_2O \) on the left side. On the right side, each \( xOH \) contributes 1 hydrogen atom. If we have 2 \( xOH \) molecules, we will have 2 hydrogen atoms, which balances the hydrogen.<br /><br />3. **Balance Oxygen (O):** <br /> Each \( H_2O \) has 1 oxygen atom, and each \( xOH \) also has 1 oxygen atom. Since we have 2 \( xOH \) molecules, we need 2 oxygen atoms, which means we need 2 \( H_2O \) molecules.<br /><br />The balanced equation is:<br /><br />\[ 2x + 2H_2O \rightarrow N_2 + 2xOH \]<br /><br />Now, let's assign coefficients:<br /><br />- For \( x \), the coefficient is 2.<br />- For \( H_2O \), the coefficient is 2.<br />- For \( N_2 \), the coefficient is 1 (or "blank" if using the provided options).<br />- For \( xOH \), the coefficient is 2.<br /><br />So, the balanced equation with coefficients is:<br /><br />\[ 2x + 2H_2O \rightarrow N_2 + 2xOH \]