Question

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 4.82×10−3s−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=4.82×10−3s−1[N2O5]2 rate=2.41×10−3s−1[N2O5] rate=4.82×10−3s−1[N2O5] rate=9.64×10−3s−1[N2O5]

Answer 1

rate = 4.82x10⁻³*[N₂O₅]

Step-by-step 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]

Answer 2

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

Step-by-step 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 ]