What is the initial rate when the initial concentrations of both reactants are 0.16M ?

Question

abb0t · Answer

You're missing quite a bit of information here I think.

abb0t · Answer

$r = k[A][B]$

anonymous · Answer

Yes I will send the rest...it was just a testing question but theres the rest of the information....
The initial rates listed in the following table were determined for the reaction 
2NO(g)+Cl2(g)→2NOCl(g) 
Experiment	 Initial [NO]	 Initial [Cl2]	 Cl2 consumption rate (initial)
1	                 0.13	0                .20	         1.0×10^−2
2	                 0.26	0                .20	         4.0×10^−2
3	                 0.13	0                .10	          5.0x10^-3
rate=k[NO]^2[Cl_2]
value of rate constant is k=3.0 /M^2 x s

anonymous · Answer

sorry for the formatting

abb0t · Answer

Well, the rate law is 2 for $NO$, so, all you're doing here is plugging in $0.16$ into the formula i provided above, solve for $r$. 

$r = k[0.16]^2[0.16]$
r = ___

anonymous · Answer

thanks a bunch!