Question #25e82

Question

Question #25e82

1 Answer

Impact of this question

8390 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2015-08-28T09:56:10

$2 K_{(s]} + H_{2} {SO}_{4(aq]} \to K_{2} {SO}_{4(aq]} + H_{2(g]}$ $2"K"_text((s]) + "H"_2"SO"_text(4(aq]) -> "K"_2"SO"_text(4(aq]) + "H"_text(2(g])$

Explanation:

Potassium metal will react with concentrated sulfuric acid to produce potassium sulfate, a salt that exists as potassium cations, $K^{+}$ $"K"^(+)$ , and sulfate anions, ${SO}_{4}^{2 -}$ $"SO"_4^(2-)$ in solution, and hydrogen gas.

The balanced chemical equation for this reaction is

$2 K_{(s]} + H_{2} {SO}_{4(aq]} \to K_{2} {SO}_{4(aq]} + H_{2(g]} ↑ ⏐$ $2"K"_text((s]) + "H"_2"SO"_text(4(aq]) -> "K"_2"SO"_text(4(aq]) + "H"_text(2(g]) uarr$

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

Science

Math

Humanities

... and beyond

Question #25e82

1 Answer

Explanation:

Related questions

Impact of this question