Questions: XCl2(aq) + AgNO3(aq) → X(NO3)2(aq) + AgCl(s)

Transcript text: $\mathrm{XCl}_{2}(\mathrm{aq})+\mathrm{AgNO}_{3}(\mathrm{aq}) \rightarrow \mathrm{X}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{AgCl}(\mathrm{s})$

Solution

Solution Steps

Step 1: Identify the Reaction Type

The given chemical equation represents a double displacement reaction, where the cations and anions of the reactants exchange partners to form new compounds. In this case, the chloride ion ($\text{Cl}^-$) from $\text{XCl}_2$ reacts with the silver ion ($\text{Ag}^+$) from $\text{AgNO}_3$ to form the insoluble precipitate $\text{AgCl}$.

Step 2: Balance the Chemical Equation

To balance the chemical equation, ensure that the number of atoms of each element is the same on both sides of the equation. The given equation is:

\[ \text{XCl}_2(\text{aq}) + \text{AgNO}_3(\text{aq}) \rightarrow \text{X}(\text{NO}_3)_2(\text{aq}) + \text{AgCl}(\text{s}) \]

Balance the silver and nitrate ions by adding a coefficient of 2 in front of $\text{AgNO}_3$ and $\text{AgCl}$:

\[ \text{XCl}_2(\text{aq}) + 2\text{AgNO}_3(\text{aq}) \rightarrow \text{X}(\text{NO}_3)_2(\text{aq}) + 2\text{AgCl}(\text{s}) \]

Step 3: Verify the Balanced Equation

Check that the number of each type of atom is equal on both sides of the equation:

Chlorine: 2 on both sides
Silver: 2 on both sides
Nitrate: 2 on both sides
X: 1 on both sides

The equation is now balanced.

Final Answer

The balanced chemical equation is:

\[ \boxed{\text{XCl}_2(\text{aq}) + 2\text{AgNO}_3(\text{aq}) \rightarrow \text{X}(\text{NO}_3)_2(\text{aq}) + 2\text{AgCl}(\text{s})} \]

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Questions: XCl2(aq) + AgNO3(aq) → X(NO3)2(aq) + AgCl(s)

Solution

Solution Steps

Final Answer

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