Question

I need help answering this question please read the question because i got it wrong twice. It says to calculate the E.Q. MOLARITY of CL2. **round the answer two decimal places**

Suppose a 250. mL flask is filled with 0.50 mol of CHCl, 1.5 mol of HCI and 1.7 mol of CCI4. The following reaction becomes possible Cl 2 (g) + CHCl 3 (g) 근 HCI (g) + CCl 4(g) The equilibrium constant K for this reaction is 0.610 at the temperature of the flask. Calculate the equilibrium molarity ofC2. Round your answer to two decimal places

Answer 1

   Cl2(g)    + CHCl3(g) ------------> HCl (g) + CCl4(g)

I                            0.5                             1.5               1.7

C           +x           +x                                -x                  -x

E            +x            0.5+x                         1.5-x            1.7-x

   [Cl2]   = x/0.25

[CHCl3] = 0.5+x/0.25

[HCl]   = 1.5-x/0.25

[CCl4]    = 1.7-x/0.25

        Kc   = (1.5-x)(1.7-x)/x*(0.5+x)

        0.61 = (1.5-x)(1.7-x)/x*(0.5+x)

     0.61*x*(0.5+x)   = (1.5-x)(1.7-x)

         x   = 0.79

      [Cl2]   = x/0.25   = 0.79/0.25   = 3.16M