The equilibrium constant, kc, for the following reaction is 5.10×10-6 at 548 k. nh4cl(s) nh3(g) + hcl(g) calculate the equilibrium concentration of hcl when 0.564 moles of nh4cl(s) are introduced into a 1.00 l vessel at 548 k.[hcl] = m

The equilibrium concentration of HCl is

Explanation:

We are given:

Moles of = 0.564 moles

Volume of vessel = 1.00 L

Molarity is calculated by using the equation:

Molarity of

The given chemical equation follows:

Initial:         0.564

At eqllm:     0.564-x          x              x

The expression of for above equation follows:

The concentration of pure solid and pure liquid is taken as 1.

We are given:

Putting values in above equation, we get:

Negative sign is neglected because concentration cannot be negative.

So,

Hence, the equilibrium concentration of HCl is

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

i have no clue hope you find the answer