Question

Write the reaction rate expressions for the reaction below in terms of the disappearance of the reactants and the appearance of products. Give the expressions for the disappearance of the reactants first, in the order written in the chemical equation. Then write the expressions for the appearance of the products in the order written in the chemical equation. Write the expressions in order of appearance in the equation in the form. ± 1 X × Δ[Α] Δt where ± is either a plus OR a minus sign, not both, X is an integer, and A is a chemical species. Do not include the state of matter. 2H2(g) + O2(g) → 2H2O(g)

Answer 1

Answer: rate of disappearance of hydrogen = $-\frac{1d[H_2]}{2dt}$   rate of disappearance of oxygen =  $-\frac{1d[O_2]}{1dt}$

rate of appearance of water = $+\frac{1d[H_2O]}{2dt}$

Explanation:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

$2H_2(g)+O_2(g)\rightarrow 2H_2O(g)$

The rate law is:

$Rate=k[H_2]^2[O_2]^1$

k= rate constant

The rate in terms of reactants is given as negative as the concentration of reactants is decreasing with time whereas the rate in terms of products is given as positive as the concentration of products is increasing with time.

rate of disappearance of hydrogen=  $-\frac{1d[H_2]}{2dt}$

rate of disappearance of oxygen = $-\frac{1d[O_2]}{1dt}$

rate of appearance of water = $+\frac{1d[H_2O]}{2dt}$