Respuesta :
Answer: The expressions are written below.
Explanation:
The rate of reaction is defined as the change in the concentration of any one of the reactants or products per unit time. For the general reaction:
[tex]rR\rightarrow pP[/tex]
Expression for the rate of reaction is given as:
[tex]\text{Rate of reaction}=\frac{\text{Decrease in the concentration of a reactant R}}{\text{Time interval}}[/tex]
Or,
[tex]\text{Rate of reaction}=\frac{\text{Increase in the concentration of a product P}}{\text{Time interval}}[/tex]
Thus,
[tex]\text{Rate of reaction}=-\frac{1}{r}\frac{\Delta [R]}{\Delta t}=+\frac{1}{p}\frac{\Delta [P]}{\Delta t}[/tex]
- For a:
The given chemical reaction follows:
[tex]H_2(g)+I_2(g)\rightarrow 2HI(g)[/tex]
Rate of the reaction for disappearance of [tex]H_2\text{ and }I_2[/tex] is given as:
[tex]\text{Rate of disappearance of }H_2=-\frac{\Delta [H_2]}{\Delta t}[/tex]
[tex]\text{Rate of disappearance of }I_2=-\frac{\Delta [I_2]}{\Delta t}[/tex]
Rate of the reaction for appearance of [tex]HI[/tex] is given as:
[tex]\text{Rate of appearance of HI}=+\frac{1}{2} \frac{\Delta [HI]}{\Delta t}[/tex]
- For b:
The given chemical reaction follows:
[tex]5Br^-(aq.)+BrO_3^{-}(aq.)+6H^+(aq.)\rightarrow 3Br_2(aq.)+3H_2O(l)[/tex]
Rate of the reaction for disappearance of [tex]Br^-,BrO_3^-\text{ and }H^+[/tex] is given as:
[tex]\text{Rate of disappearance of }Br^-=-\frac{1}{5} \frac{\Delta [Br^-]}{\Delta t}[/tex]
[tex]\text{Rate of disappearance of }BrO_3^-=-\frac{\Delta [BrO_3^-]}{\Delta t}[/tex]
[tex]\text{Rate of disappearance of }H^+=-\frac{1}{6} \frac{\Delta [H^+]}{\Delta t}[/tex]
Rate of the reaction for appearance of [tex]Br_2\text{ and }H_2O[/tex] is given as:
[tex]\text{Rate of appearance of }Br_2=+\frac{1}{3} \frac{\Delta [Br_2]}{\Delta t}[/tex]
[tex]\text{Rate of appearance of }H_2O=+\frac{1}{3} \frac{\Delta [H_2O]}{\Delta t}[/tex]
Hence, the expressions are given above.
The reaction rate expressions for the given reactions are:
r = -Δ[H₂(g)] / Δt = -Δ[I₂(g)] / Δt = Δ[HI(g)] / 2 Δt
r = -Δ[Br⁻(aq)] / 5 Δt = -Δ[BrO₃⁻(aq)] / Δt = -Δ[H⁺(aq)] / 6 Δt = Δ[Br₂(aq)] / 3Δt = Δ[H₂O(l)] / 3 Δt
What is the reaction rate?
The reaction rate is the speed at which a chemical reaction takes place, defined as proportional to the increase in the concentration of a product per unit time and to the decrease in the concentration of a reactant per unit time.
To write the reaction rate expression, we have to:
- Express the change in the concentration of the species over time.
- Add a negative sign if the species is a reactant.
- Divide by the stoichiometric coefficient of the species.
a. H₂(g) + I₂(g) → 2 HI(g)
r = -Δ[H₂(g)] / Δt = -Δ[I₂(g)] / Δt = Δ[HI(g)] / 2 Δt
b. 5 Br⁻(aq) + BrO₃⁻(aq) + 6 H⁺(aq) → 3 Br₂(aq) + 3 H₂O(l)
r = -Δ[Br⁻(aq)] / 5 Δt = -Δ[BrO₃⁻(aq)] / Δt = -Δ[H⁺(aq)] / 6 Δt = Δ[Br₂(aq)] / 3Δt = Δ[H₂O(l)] / 3 Δt
The reaction rate expressions for the given reactions are:
r = -Δ[H₂(g)] / Δt = -Δ[I₂(g)] / Δt = Δ[HI(g)] / 2 Δt
r = -Δ[Br⁻(aq)] / 5 Δt = -Δ[BrO₃⁻(aq)] / Δt = -Δ[H⁺(aq)] / 6 Δt = Δ[Br₂(aq)] / 3Δt = Δ[H₂O(l)] / 3 Δt
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