Can anyone tell me why the answer that I got here is not correct?
Pb(s) + AgNO3(aq)
yields Ag(s) + PbNO3(s)
Pb will go to lead(II), valence +2
Is it still a single displacement reaction? can you walk me through predicting the reaction and then balancing it. I'm lost.
I don't think you picked up on the problem from the answer by Bob P. You have the wrong formula for lead(II) nitrate. It is written Pb(NO3)2
To understand why the answer you got might not be correct, we need to analyze the given chemical equation:
Pb(s) + AgNO3(aq) → Ag(s) + PbNO3(s)
This equation represents a reaction between solid lead (Pb) and aqueous silver nitrate (AgNO3). The products of the reaction are solid silver (Ag) and solid lead nitrate (PbNO3).
To determine if the answer is correct or not, you need to consider the laws of chemical reactions, specifically the law of conservation of mass. According to this law, matter is neither created nor destroyed in a chemical reaction. Therefore, the total mass of the reactants should be equal to the total mass of the products.
In this equation, we have one mole of silver nitrate reacting with one mole of lead. The products are one mole of silver and one mole of lead nitrate. To check if the equation is balanced, we need to compare the number of atoms on both sides:
On the reactant side:
- There is one atom of lead (Pb).
- There is one atom of silver (Ag).
- There is one atom of nitrogen (N).
- There are three atoms of oxygen (O).
On the product side:
- There is one atom of silver (Ag).
- There is one atom of lead (Pb).
- There is one atom of nitrogen (N).
- There are three atoms of oxygen (O).
Since the number of atoms is the same on both sides, the equation is balanced.
If the answer you obtained is different from this chemical equation, it might be due to an error in balancing the equation or misunderstanding the reactants and products. Double-check your calculations and make sure that you correctly identify the chemical species involved in the reaction.