The following reaction is first order in N2O5: N2O5 (g) →NO3 (g) + NO2 (g) The rate constant for the reaction at a certain temperature is 0.053/s

Calculate the rate of the reaction when [N2O5] = 5.1*10-2 M.

What would the rate of the reaction be at the same concentration as in Part A if the reaction were second order?

What would the rate of the reaction be at the same concentration as in Part A if the reaction were zero order?

1) 2.703 x 10⁻³ M/s.

2) 1.378 x 10⁻⁴ M/s.

3) 0.053 M/s.

Explanation:

1) Calculate the rate of the reaction when [N₂O₅] = 5.1*10⁻² M.

For a first order reaction:

The rate of the reaction = k[N₂O₅],

where, k is the rate constant of the reaction (k = 0.053 s⁻¹).

[N₂O₅] is the concentration of the reactant ([N₂O₅] = 5.1 x 10⁻² M).

∴ The rate of the reaction = k[N₂O₅] = (0.053 s⁻¹) (5.1 x 10⁻² M) = 2.703 x 10⁻³ M/s.

2) What would the rate of the reaction be at the same concentration as in Part A if the reaction were second order?

For a second order reaction:

The rate of the reaction = k[N₂O₅]²,

where, k is the rate constant of the reaction (k = 0.053 M⁻¹s⁻¹).

[N₂O₅] is the concentration of the reactant ([N₂O₅] = 5.1 x 10⁻² M).

∴ The rate of the reaction = k[N₂O₅]² = (0.053 M⁻¹s⁻¹) (5.1 x 10⁻² M) ² = 1.378 x 10⁻⁴ M/s.

3) What would the rate of the reaction be at the same concentration as in Part A if the reaction were zero order?

For a zero order reaction:

The rate of the reaction = k[N₂O₅]⁰,

where, k is the rate constant of the reaction (k = 0.053 M/s).

[N₂O₅] is the concentration of the reactant ([N₂O₅] = 5.1 x 10⁻² M).

∴ The rate of the reaction = k[N₂O₅]⁰ = (0.053 M/s) (5.1 x 10⁻² M) ⁰ = 0.053 M/s.