The first reaction is correct and correctly balanced. It is a single replacement.
The second one shown is correct and balanced. With some reservations this is a double replacement; however, it isn't a good example of a Double Replacement(DR). By definition a DR in this case would produce Ba(NO3)2 + NH4OH and many links on Google correctly show that NH4OH DECOMPOSES (remember decomposition is another type of chemical reaction) into NH3 and H2O. However, it has been shown that NH4OH does not exist. That is a solution of NH3 gas in water is just that; i.e., NH4 gas and water. No NH4OH is every formed; therefore, to call it a decomposition isn't quite right which makes the DR moniker not quite right either. Go with what your teacher has taught you. I'm not trying to confuse you; I just don't want you using the NH4OH and then decomposing as an argument since NH4OH doesn't exist. I should note here that whether NH4OH actually exists is a hotly debated subject. I base my opinion on the fact that the spectrum of NH3 gas dissolved in water contains no new absorption bands.
I have a chem project and I did the work but I’m not sure if I’m correct or not.
1. Our reactants were: Calcium and Water and we have to balance the equation and write what type of reaction it was.
I got Ca+2H2O ——> Ca(OH)2 + H2 and a single replacement
2. Our other reactants were: ammonium nitrate and barium hydroxide and again we had to balance the equation and write what type of reaction it was.
I got 2Nh4NO3+Ba(OH)2 ——-> Ba(NO3)2 + 2H2O + 2NH3 and a double replacement
I just want to know if I’m on the right track!
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