Rate Law from Initial Rates (B) - Chemistry help?
The above reaction was studied (at a particular temperature) and the following data (for rate = -d[ClO2]/dt) were obtained:
[ClO2]0 [OH-]0 Initial Rate
(mol/L) (mol/L) (mol L-1 s-1)
0.150 0.050 2.52×10-1
0.300 0.050 1.01
0.300 0.025 5.04×10-1
Which of the following expressions for the rate law are consistent with the above experimental data.
Note that the rate constant may be different for each of the choices below (i.e. k in choice A may be not equal to k in choice B etc).
k[ClO2]2[OH-] = -d[OH-]/dt ( i put yes)
k[ClO2]2[OH-] = d[ClO3-]/dt (i put yes)
-d[OH-]/dt = k[OH-][ClO2-]2 (i put yes)
k[ClO2]2[OH-] = d[ClO2-]/dt ( i put no)
k[ClO2][OH-]2 = -d[OH-]/dt (i put no)
i keep getting it incorrect, anyone please help me out?