# Question #25e82

Aug 28, 2015

$2 {\text{K"_text((s]) + "H"_2"SO"_text(4(aq]) -> "K"_2"SO"_text(4(aq]) + "H}}_{\textrm{2 \left(g\right]}}$

#### Explanation:

Potassium metal will react with concentrated sulfuric acid to produce potassium sulfate, a salt that exists as potassium cations, ${\text{K}}^{+}$, and sulfate anions, ${\text{SO}}_{4}^{2 -}$ in solution, and hydrogen gas.

The balanced chemical equation for this reaction is

$2 {\text{K"_text((s]) + "H"_2"SO"_text(4(aq]) -> "K"_2"SO"_text(4(aq]) + "H}}_{\textrm{2 \left(g\right]}} \uparrow$

This is a very strong redox reaction in which potassium is being oxidized and hydrogen is being reduced.