The decomposition of N2O5 in carbon tetrachloride proceeds as follows: 2N2O5→4NO2+O2 The rate law is first order in N2O5. At 64 ∘C the rate constant is 4.8210-3s-1. You may want to reference (Pages 576 - 581) Section 14.3 while completing this problem. Part A Which of the following is the rate law for this reaction? Which of the following is the rate law for this reaction? rate=4.8210-3s-1[N2O5]2 rate=2.4110-3s-1[N2O5] rate=4.8210-3s-1[N2O5] rate=9.64*10-3s-1[N2O5]

Question

Andrew Long

Chemistry

21 August, 14:52

The decomposition of N2O5 in carbon tetrachloride proceeds as follows: 2N2O5→4NO2+O2 The rate law is first order in N2O5. At 64 ∘C the rate constant is 4.8210-3s-1. You may want to reference (Pages 576 - 581) Section 14.3 while completing this problem. Part A Which of the following is the rate law for this reaction? Which of the following is the rate law for this reaction? rate=4.8210-3s-1[N2O5]2 rate=2.4110-3s-1[N2O5] rate=4.8210-3s-1[N2O5] rate=9.64*10-3s-1[N2O5]

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Answers (2)

Know the Answer?

Isabelle Richmond · Answer 1

r = 2.41 E-3 s-1 [ N2O5 ]

Explanation:

2N2O5 → 4NO2 + O2

∴ k = 4.82 E-3 s-1

⇒ r = k [ N2O5 ]/2

⇒ r = (4.82 E-3 s-1 [ N2O5 ]) / 2

⇒ r = 2.41 E-3 s-1 [ N2O5 ]

Salas · Answer 2

rate = 4.82x10⁻³*[N₂O₅]

Explanation:

The rate of a reaction represents how much moles of the reactant is disappearing along the time, and for a reaction with only one reactant, it can be calculated by:

rate = k*[reactant]ⁿ

Where k is the rate constant, [reactant] is the initial concentration of the reactant, and n is the order of the reaction, which is determined by experiments. So, if the rate law is first order, n = 1:

rate = 4.82x10⁻³*[N₂O₅]