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]

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

Explanation:

∴ 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 ]

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]