Complete this br? nsted-lowry reaction, placing each product by its appropriate label. hso4(1-)+cn(1-)

Based on the Bronsted-Lowry theory:

An acid is defined as a species which in solution tends to lose a proton (H+) while base is a species that tends to accept protons.

The given situation, HSO4⁻ acts as an acid and loses its H+ to CN⁻.

HSO4⁻ + CN⁻↔ SO4²⁻ + HCN

Here, HSO4⁻ is the acid while SO4²⁻ is its conjugate base

CN⁻ is a base and HCN is its conjugate acid

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

24