Question

Be sure to answer all parts. Write the balanced equations corresponding to the following rate expressions: a) rate = − 1 3   Δ[CH4] Δt = − 1 2   Δ[H2O] Δt = − Δ[CO2] Δt = 1 4   Δ[CH3OH] Δt (Click in the answer box to activate the palette. Do not include states of matter.) b) rate = − 1 2   Δ[N2O5] Δt = 1 2   Δ[N2] Δt = 1 5   Δ[O2] Δt (Click in the answer box to activate the palette. Do not include states of matter.) c) rate = − 1 2   Δ[H2] Δt = − 1 2   Δ[CO2] Δt = − Δ[O2] Δt = 1 2   Δ[H2CO3] Δt

Answer 1

Sol :-

The given overall rate is equal to the rate of reaction with respect to each reagent in which stoichiometric coefficients with respect to each reagents are divided.

For Reactants :-

Rate = - Change in concentration of reactant (- Δ [R] ) / change in time  (Δt )

Here, -ve sign indicates that concentration of reactants decreases with time.

For Products :-

Rate = + Change in concentration of products (- Δ [P] ) / change in time  (Δt )

Here, +ve sign indicates that concentration of products increases with time.

(a). rate = − 1 / 3   Δ[CH₄] Δt = − 1 / 2   Δ[H₂O] Δt = − Δ[CO₂] Δt = 1/ 4   Δ[CH₃OH] Δt

The balance equation is :

3 CH₄ + 2 H₂O + CO₂ ------------------> 4 CH₃OH

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(b). rate = − 1 / 2   Δ[N₂O₅] Δt = 1 / 2   Δ[N₂] Δt = 1 / 5   Δ[O₂] Δt

The balance equation is :

2 N₂O₅ ----------------> 2 N₂ + 5 O₂

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(c). rate = − 1 / 2   Δ[H₂] Δt = − 1 / 2   Δ[CO₂] Δt = − Δ[O₂] Δt = 1 / 2   Δ[H₂CO₃] Δt

The balance equation is :

2 H₂ + 2 CO₂ + O₂ ----------------> 2 H₂CO₃