A.)the equilibrium constant, kp, for the following reaction is 0.110 at 298 k:
nh4hs(s) nh3(g) + h2s(g)
calculate the equilibrium partial pressure of h2s when 0.371 moles of nh4hs(s) is introduced into a 1.00 l vessel at 298 k.
ph2s = ? ? atm
b.) the equilibrium constant, kp, for the following reaction is 0.497 at 500 k:
pcl5(g) pcl3(g) + cl2(g)
calculate the equilibrium partial pressures of all species when pcl5(g) is introduced into an evacuated flask at a pressure of 1.47 atm at 500 k .
ppcl5 = ? ? atm
ppcl3 = ? ? atm
pcl2 = ? ? atm

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.

my dad did alot of meth and ace cheeks