Question
can you please show all your steps. I am lost
dure Im the cete andgt EXAMPLE 14.4 EXAMPLE 14.5 Finding Equilibrium Constants Finding Equilibrium Constants from Experimental Partial Pressure Measurements from Experimental Concentration Measurements Consider the following reaction: cog) + 2 H2(g)- CH,OH(g) Consider the following reaction: | Ni(s) + 2 V3+ (aq)--Ni2+(aq) + 2 V2+(aq) A reaction mixture at 400 K initially A chunk of solid nickel is placed into a contained CO and H2 at partial pressures 0.250 mol L- solution of V+ at 298 K. At of 0.750 and 1.000 bar, respectively. At equilibrium the concentration of V was equilibrium, the partial pressure of CO found to be 0.056 mol L-1. What is the value of was found to be 0.295 bar. What is the the equilibrium constant? value of the equilibrium constant?
Explanation / Answer
Ans 14.4
Balanced equation with ICE table
CO + 2H2 = CH3OH
I 0.75 1 -
C - x - 2x +x
E 0.75 - x 1-2x x
At equilibrium
Partial pressure of CO = 0.295 bar
0.75 - x = 0.295
x = 0.455 bar
At equilibrium
Partial pressure of H2 = 1 - 2x = 1 - 2*0.455 = 0.09 bar
Partial pressure of CH3OH = x = 0.455 bar
Equilibrium constant
Kp = pCH3OH /(pH22 pCO)
= 0.455/(0.09*0.09*0.295)
Kp = 190.416