hslove142331
Mar 3, 2010, 04:13 PM
At 25 °C, Kc= 0.145 for the following reaction in the solvent CCl4.
2BrCl <------------> Br2+Cl2
If the initial concentrations of Br2 and Cl2 are each 0.0195 M, what will their equilibrium concentrations be?
I tried 4 times.. but my answers were all wrong. I have only one chance to get correct.
I don't know I did like this.
(0.0195-x)^2/(2x)^2=0.145
0.0195-x=0.7616x
x=0.011
M=0.0085, right?
I am not sure even I didn't try to put that unsure answer.
So please please help me
And I am so confusing on I/C/E steps.
I know I and E
But I don't know how to figure Out on C that which side have(-)or(+)
Please help me Thanks
2BrCl <------------> Br2+Cl2
If the initial concentrations of Br2 and Cl2 are each 0.0195 M, what will their equilibrium concentrations be?
I tried 4 times.. but my answers were all wrong. I have only one chance to get correct.
I don't know I did like this.
(0.0195-x)^2/(2x)^2=0.145
0.0195-x=0.7616x
x=0.011
M=0.0085, right?
I am not sure even I didn't try to put that unsure answer.
So please please help me
And I am so confusing on I/C/E steps.
I know I and E
But I don't know how to figure Out on C that which side have(-)or(+)
Please help me Thanks