Use the activity series of metals to write a balanced chemical equation for each single-replacement reaction.
Zn(s) + AgNO3 (aq) -->
NOTE: The three above is a subscript...it should be a small 3.
Please explain how to figure out this problem, and provide a thorough explanation on how I have to consider the activity series of metals.
A displacement will only take place if the free metal is higher on the activity series than in the bond.
Since Zn is higher on the activity series than Ag a reaction takes place and it becomes ZnNO3 + Ag
Answer: Zn + 2AgNO3 --> Ag+ Zn(NO3)2
To balance the chemical equation for the given single-replacement reaction, you need to consider the activity series of metals. The activity series is a list of metals in order of their reactivity, with the most reactive metals at the top and the least reactive ones at the bottom.
In this case, zinc (Zn) is a more reactive metal than silver (Ag) according to the activity series. This means that zinc can replace silver in a chemical reaction, but not vice versa.
To balance the equation, you need to ensure that the number of atoms of each element is the same on both sides. Follow these steps:
Step 1: Write out the reactants and products.
Zn(s) + AgNO3(aq) -->
Step 2: Identify the elements present on both sides of the equation.
The reactants have zinc (Zn) and the products have silver (Ag) and nitrogen (N).
Step 3: Determine which element will be replaced.
Since zinc is more reactive than silver, it will replace the silver in the compound AgNO3.
Step 4: Write the balanced equation by exchanging the metals.
Zn(s) + AgNO3(aq) → Zn(NO3)2(aq) + Ag(s)
Step 5: Check that the equation is balanced.
Count the number of each type of atom on both sides of the equation:
Reactants: 1 zinc (Zn) atom, 1 silver (Ag) atom, 1 nitrogen (N) atom, and 3 oxygen (O) atoms
Products: 1 zinc (Zn) atom, 2 nitrogen (N) atoms, 6 oxygen (O) atoms, and 1 silver (Ag) atom
Now, the equation is balanced, with the same number of each type of atom on both sides.
To write a balanced chemical equation for the single-replacement reaction, you need to consider the activity series of metals. The activity series lists metals in order of their reactivity, with the most active (or reactive) metals at the top and the least active metals at the bottom.
In the given reaction, you have zinc (Zn) and silver nitrate (AgNO3). To determine if a reaction will occur, you compare the reactivity of the two metals involved. Zinc is higher on the activity series than silver. Therefore, we can predict that a reaction will occur, with zinc displacing silver.
To write the balanced chemical equation, follow these steps:
1. Write the reactants: Zn(s) + AgNO3(aq)
- Zn(s) represents solid zinc metal.
- AgNO3(aq) represents aqueous silver nitrate.
2. Identify the products: The zinc will replace the silver in silver nitrate, producing zinc nitrate (Zn(NO3)2) and solid silver (Ag).
3. Write the products: Zn(s) + AgNO3(aq) → Zn(NO3)2(aq) + Ag(s)
- Zn(NO3)2(aq) represents aqueous zinc nitrate.
- Ag(s) represents solid silver.
4. Balance the equation: The equation is already balanced in terms of atoms. However, you can verify that the equation is balanced by ensuring that the number of each type of element is the same on both sides of the equation.
And that's how you use the activity series of metals to write a balanced chemical equation for a single-replacement reaction!