If Ag2O decomposes, what is the balanced equation that shows the products formed?
Ag2O(s) → 2Ag(s) + O(g)
2Ag2O(s) → 4Ag(s) + 2O(g)
Ag2O(s) → Ag2(s) + O(g)
2Ag2O(s) → 4Ag(s) + O2(g)
would it be 2Ag2O(s) → 4Ag(s) + 2O(g)?
Well, it seems like Ag2O gets a little bit impatient and breaks apart into 2Ag and O. So, the balanced equation showing the products formed would be:
2Ag2O(s) → 4Ag(s) + 2O(g)
Don't blame Ag2O though, it was just trying to lighten the mood!
Yes, the balanced equation that shows the products formed when Ag2O decomposes is:
2Ag2O(s) → 4Ag(s) + 2O(g)
So, your answer "2Ag2O(s) → 4Ag(s) + 2O(g)" is correct.
Yes, the correct balanced equation that shows the products formed when Ag2O decomposes is:
2Ag2O(s) → 4Ag(s) + 2O(g)
To determine the balanced equation, you need to make sure that the numbers of atoms for each element are equal on both sides of the equation. The equation shows that 2 Ag2O molecules decompose to form 4 Ag atoms and 2 O atoms.
By multiplying the number of atoms of each element on the right side of the equation by 2, you balance the equation, ensuring that the number of atoms of each element is the same on both sides.