Answer : All of the above are valid expressions of the reaction rate.
Explanation :
The given rate of reaction is,
[tex]4NH_3+7O_2\rightarrow 4NO_2+6H_2O[/tex]
The expression for rate of reaction for the reactant :
[tex]\text{Rate of disappearance of }NH_3=-\frac{1}{4}\times \frac{d[NH_3]}{dt}[/tex]
[tex]\text{Rate of disappearance of }O_2=-\frac{1}{7}\times \frac{d[O_2]}{dt}[/tex]
The expression for rate of reaction for the product :
[tex]\text{Rate of formation of }NO_2=+\frac{1}{4}\times \frac{d[NO_2]}{dt}[/tex]
[tex]\text{Rate of formation of }H_2O=+\frac{1}{6}\times \frac{d[H_2O]}{dt}[/tex]
From this we conclude that, all the options are correct.
Based on the equation of the reaction, all of the given expressions are valid expressions of the reaction rate.
The rate of a chemical reaction is the rate at which reactants are used up or the rate at which products are formed.
The rate of a reaction is obtained from the balanced equation of the reaction.
The equation of the reaction is given below:
Rate of disappearance of NH3 = - 1/4 × Δ[NH3]/Δt
Rate of disappearance of O2 = - 1/7 × Δ[O2]/Δt
Rate of formation of NO2 = 1/4 × Δ[NO2]/Δt
Rate of formation of H2O = 1/6 × Δ[H2O]/Δt
Therefore, all of the above are valid expressions of the reaction rate.
Learn more about rate of reaction at: https://brainly.com/question/24795637
