You plugged in mols and not concentration.
Initial (HI) = 0.4/0.5 = ?
Initial (I2) = 1.6/0.5 = ?
Suppose a 500mL flask is filled with 1.6 mol of I2 and 0.40 mol of HI.
The following reaction becomes possible:
H2(g)+I2(g) -----> 2HI(g)
The equilibrium constant K for this reaction is 0.923 at the temperature of the flask.
Calculate the equilibrium molarity of H2.
Ive gotten up to
K = [HI]^2/[H2][I2] = 0.923
0.923 = (0.4-2x)^2/(x)(1.6+x)
Im aware quadratic formula is needed to solve this however I am still not getting to correct answer when I try solve for x.
1 answer
1 answer