Does the concentration of water accounts for determining the rate of a reaction?
Rate law vs. definition of rate

For this problem, you don't need the rate law. And, just for the record, you can't get the rate law from the stoichiometry - it depends on the mechanism and has to be determined empirically.

Definition of rate of reaction

The rate of reaction is based on the change of concentrations. For a homogeneous reaction (i.e. all species in the same gas phase, or all species part of the same solution), the definition is the following:

$$\mathrm{rate} = \frac{d[\ce{X}]}{\nu_X \cdot dt}$$

where $\nu_X$ is the stoichiometric coefficient of the species $\ce{X}$. This does not apply to heterogeneous reactions. For one, if a species is a pure solid or liquid, its concentration will not change. Also, the stoichiometry of a reaction refers to amount of substance - only if all species are in the same solution (or the same gas phase) does this translate into easy relationships of concentration changes (or partial pressure changes).

Definition of "rates of the chemical species"

This is not a technical term I am familiar with. In order to be able to answer the question with answer 3., you would have to define it as:

$$v_\ce{X} = \frac{\mid dn_\ce{X} \mid}{dt}$$

Once you define it such, it does not matter what the physical state of reactants and products is, it does not matter whether a species is a reactant or a product, the only thing you need to related the different rates are the stoichiometric coefficients.

So for example, the ratio of the amount of hydrogen and oxygen used is equal to the ratio of stoichiometric coefficients:

$$\frac{\Delta n_\ce{H2}}{\Delta n_\ce{O2}} = \frac{\nu_\ce{H2}}{\nu_\ce{O2}} = \frac{2}{1}$$