Question

I keep getting the wrong answer for this one can someone help. The initial concentration for the compounds involved in the reaction displayed were determined to be [NOCl(g)] = 0.1738 mol/L, [NO(g)] = 0.1991 mol/L, [Cl2(g)] = 0.000005938 mol/L. Calculate the value of the equilibrium constant (Kc) at 25.00 °C if the equilibrium concentration of NO(g) was 0.1991 mol/L.

2NOCl(g) = 2NO(g)+Cl2(g)

Answer 1

I can't possibly find your error without your work. It is an odd problem that has initial and final concentrations the same. Are you certain this is the problem?


keq= (.1991)^2 *(5.938E-7)/(.1738)^2