Suppose a flask is filled with of , of and of. the following reaction becomes possible: the equilibrium constant for this reacti

Question

zubka84 [21]

2 years ago

14

Suppose a flask is filled with of , of and of. the following reaction becomes possible: the equilibrium constant for this reacti

on is at the temperature of the flask. calculate the equilibrium molarity of. round your answer to two decimal places

SAT

1 answer:

AlladinOne [14] · Answer 1 · 2023-04-09T06:05:03+03:00

The concentrations of the species at equilibrium is obtained from the ICE table.

<h3>What is equilibrium constant?</h3>

The equilibrium constant shows the extent to which a reactant has been converted into products. A large equilibrium constant means that most of the reactants are converted into products The question is incomplete as the details as missing.

However, for a hypothethical reaction; nA + mB ⇄ xC + zD, the equilibrium constant is obtained from; K = [C]^x [D]^z/[A]^n [B]^m. The concentrations of the species at equilibrium is obtained from the ICE table.

Learn more about equilibrium: brainly.com/question/10038290