kinetic reaction rate greater than extent of reaction for equilibrium

I'm comparing a model with chemistry at equilibrium versus a kinetic one.  

I take a network of two reactions: methane steam reforming (MSR) and water gas shift (WGS) at 700°C. 


I calculated extent of reaction of both reaction, with the equilibrium hypothesis, solving a system of two non-linear equation containing the two $ K \_{eq} (T) =f(\lambda\_{MSR}, \lambda\_{WGS}) $ equations, which give me these results: 


$\lambda\_{MSR} = 1.4167e-4 [mol/s]$  

 $\lambda\_{WGS} = -6.6788e-5 [mol/s]$ 


Then I calculate rates of reaction with an homogeneous and stoichiometric coefficient expression, with Temperature dependence constant (Arrhenius) taken [here](http://dx.doi.org/10.1016/j.ijheatmasstransfer.2004.04.010), I get: 


$r \_{MSR} = 20.9761e-4 [mol/s/m^3]$  

 $r \_{WGS} = 0.0 [mol/s/m^3]$ (I have no reactants nor products...) 


Now to compare them I have to multiply $r$ for reactor's volume. 


Here start my doubt:  

taking for sake of simplicity $1[m^3]$ reactor, I get 



> 
> $r\_{MSR}>\lambda\_{MSR}$ 
> 
> 
> 


* this what does it mean?
* does it have a physical meaning?
* what is the meaning of a so large reactor?


My thoughts, my idea, is that equilibrium shows the maximum rate of reaction so kinetic should, or better must, respect it giving me a lower value of reaction rate; but, as you can easily see in my above example, this ***statement*** (that I have never read somewhere in any chemistry book, so I can take it as ***truth***) can be superimposed, forced. How do you explain it?


