Ask Me Help Desk - Chemical reactions

Are the products of calcium + water --- calcium hydroxide + hydrogen gas and is that expressed as CaOH + H2O ----(arrow) CaOH + H2

Are the products of tin + antimony(V)chloride----tin chloride + antimony
And is that expressed as Sn + AtCl5-----(arrow) SnCl5 + At

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Are the products of calcium + water --- calcium hydroxide + hydrogen gas and is that expressed as $Ca + H_2O \rightarrow CaOH + H_2\,?$

Are the products of tin + antimony(V)chloride----tin chloride + antimony
and is that expressed as $Sn + SbCl_5 \rightarrow SnCl_5 + At$

Calcium hydroxide is $Ca(OH)_2$ and not $Ca(OH)$ . Calcium does react with water to form calcium hydroxide and hydrogen:

$Ca + 2\,H_2O \rightarrow Ca(OH)_2 + H_2$

Antimony is Sb, not At (astatine).

I think the reaction you want is $Sn + SbCl_5 \rightarrow SnCl_5 + Sb$

I didn't look up the chemical potentials of tin and antimony, but I think that tin will replace antimony as shown. The pentachlorides aren't that common. The trichlorides are more common and more stable.

Reaction between ammonium corbonate and sulphuric acid

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Originally Posted by mrunal_moh

Reaction between ammonium carbonate and sulphuric acid

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$(NH_4)_2CO_3 + H_2SO_4 \rightarrow 2NH_4^+ + CO_3^{-2} + 2H^+ SO_4^{-2} \rightarrow$

What I've written is the ionization of both species. It would stay like that (a mixture of ions) unless something drives the reaction to the right. Something that might drive the reaction to the right would be that something was removed from the solution. For example, something might precipitate. If you combine the anions with the cations, will anything precipitate? (Use your solubility rules to figure that out). Another thing that might drive the reaction to the right would be something that decomposes. If something decomposed to produce a gas, and that gas bubbled out of the solution, that would drive the reaction to the right. Again, combine the anions with the cations. Will any of those compounds decompose to produce a gas? (Hint: yes).