# How would one write balanced chemical, complete ionic, and net ionic equations for the reactions between the following substances, which produce a gas?

## a. hydrochloric acid and aqueous sodium cyanide, with production of hydrogen cyanide gas (HCN) b. sulfuric acid (H2SO4) and aqueous rubidium sulfide, with production of hydrogen sulfide gas Thank you for trying to help me out! Let's just say that chemistry is not my strongest subject! :)

Apr 5, 2017

$a .$ $H C l \left(a q\right) + N a C \equiv N \left(a q\right) \rightarrow H C \equiv N \left(g\right) \uparrow + N a C l \left(a q\right)$

#### Explanation:

And ths would be a dangerous reaction to do, in that you produce volatile hydrogen cyanide........

$b .$ ${H}_{2} S {O}_{4} \left(a q\right) + R {b}_{2} S \left(a q\right) \rightarrow {H}_{2} S \left(g\right) \uparrow + R {b}_{2} S {O}_{4} \left(a q\right)$

And this would be a bit less dangerous, but still hydrogen sulfide is mighty smelly.

We write $\left(a q\right)$ to represent the $\text{aquated ion}$ in aqueous solution. For instance $N a C l \left(a q\right)$ would probably be the aquated ions, ${\left[N a {\left(O {H}_{2}\right)}_{6}\right]}^{+}$ and ${\left[C l {\left({H}_{2} O\right)}_{4 - 6}\right]}^{-}$.

When we write $H C l \left(a q\right)$, in solution we likely have ${H}_{3} {O}^{+}$ (or a cluster of water molecules with an extra ${H}^{+}$), and chloride ion, $C {l}^{-}$, which again is surrounded by, or solvated by several water molecules.

And as a result the net ionic equations are:

$c .$ H_3O^+ +""^(-)C-=N rarr HC-=N(g)uarr + H_2O(l)

$d .$ $2 {H}_{3} {O}^{+} + {S}^{2 -} \rightarrow {H}_{2} S \left(g\right) + 2 {H}_{2} O \left(l\right)$

You will have to supply the chemical equations..........