If 0.500 mol of iodine and 0.500 mol of chlorine are initially placed into a 2.00-L reaction vessel at 25°C, find the concentrations of all entities at equilibrium.
I2(g) + Cl2(g) ⇌ 2 ICl(g) K = 81.9 at 25°C
"I_{2(g) } + Cl_{2(g) }\u21cc 2 ICl_{(g) }"
I: 0.500mol + 0.500mol = 0mol
C: -xmol + -xmol = +xmol
E: 0.500-x mol + 0.500-x = x
"K_c =\\dfrac{x\u00b2}{(0.500-x)(0.500-x)}"
"81.9 =\\dfrac{x\u00b2}{(0.500-x)(0.500-x)}"
"81.9 ( 0.250- x +x\u00b2) = x\u00b2"
"20.475 -81.9x+ 81.9x\u00b2 = x\u00b2"
"80.9x\u00b2- 81.9x +20.475 = 0"
x = 0.45 or 0.56, but the value of K is greater than 1, so product conc. > reactant conc.
"\\therefore x=0.56M"
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