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.

the earth would become to overheated and everything alive on it will eventually die from overheating. plants will eventually die as well, water will evaporate, and it will be nothing but a hot planet without anything living on it.