[Serenagreene]

What am I doing wrong?  My answers don't match the teachers..

1.00 g of each NO2(g) and Cl2 (g) are placed in an empty 100-mL flask and allowed to reach equilibrium via the following reaction:  2NO(g) + Cl2(g) <--> 2 NOCl(g).  The K value of the reactions is 6.25 * 10^4 L/mol

 
          [NOCl]^2
K =   --------------------
        [NO]^2 * [Cl2]
     
[NO] = 1g/30.1 g/mol = 0.0332 mol /.1 l = .332 M
[Cl2] = 1g/70.91 g/mol = 0.0141 mol / .1l = .141 M



S                     I                         C                        E
NO               .332                      2x                       .332- 2x
Cl2               .141                       x                        .141 - x
NOCl             0                         2x                         2x

6.25 * 10^4 = (2x)^2/[(.332 - 2x)^2*(.141 - x)]
x = 0.1405

at equilibrium
[NO] = 0.051 M
[Cl2] = 0.0005M
[NOCl2] = 0.281 M

teacher's answers were: 

[NO] = 0.00392 M
[Cl2] = 0.117 M
[NOCl2] = 0.329 M

[xiankai]

are you given NO₂ or NO?
is NOCl or NOCl₂ produced?
you have several conflicting statements, and you should check the question properly first

[Serenagreene]

Sorry it was NO that was given.  But I did use the correct rxn equation given

2NO + Cl2 <--> 2 NOCl