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?

When [N₂O₅] = 5.1 × 10⁻² M, the first-order decomposition of N₂O₅ has a reaction rate of 2.7 × 10⁻² M/s. If it were of second order, the reaction rate would be 1.4 × 10⁻⁴ M/s. If it were of zero order, the reaction rate would be 0.053 M/s.

Let's consider the following reaction.

N₂O₅(g) → NO₃(g) + NO₂(g)

This reaction is of first order with a rate constant (k) of 0.053/s. We can calculate the rate of the reaction when [N₂O₅] = 5.1 × 10⁻² M using the first-order rate law.

For the same concentration and numerical value of the rate constant, if the reaction were of second order, we would use the second-order rate law.

For the same concentration and numerical value of the rate constant, if the reaction were of zero order, we would use the zero-order rate law.

When [N₂O₅] = 5.1 × 10⁻² M, the first-order decomposition of N₂O₅ has a reaction rate of 2.7 × 10⁻² M/s. If it were of second order, the reaction rate would be 1.4 × 10⁻⁴ M/s. If it were of zero order, the reaction rate would be 0.053 M/s.

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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.

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?

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?

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.

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