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antiseptic1488 [7]
3 years ago
10

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. Part A Part complete Write the rate law for the reaction. Write the rate law for the reaction. rate=2.41×10−3s−1[N2O5] rate=4.82×10−3s−1[N2O5] rate=9.64×10−3s−1[N2O5] rate=4.82×10−3s−1[N2O5]2 Previous Answers Correct Part B What is the rate of reaction when [N2O5]= 2.80×10−2 M ?
Chemistry
1 answer:
Nesterboy [21]3 years ago
8 0

Answer:

Part A

rate= 4.82*10^{-3}s^{-1} * [N2O5]

Part B

rate= 1.35*10^{-4}Ms^{-1}

Explanation:

Part A

<em>The rate law is the equation that relates the rate of the reaction, the kinetic constant and the concentration of the reactant or reactants.</em>

For the given chemical reaction we can write a general expression for the rate law as follows:

rate= k * [N2O5]^{x}

where k is the rate constant and x is the order of the reaction with respect of N2O5 concentration. Particularly, <em>a first order reaction kinetics indicate that the rate of the reaction is directly proportional to the concentration of only one reactant</em>. Then x must be 1.

Replacing the value of the rate constant given in the text we can arrive to the following expression for the rate law:

rate= 4.82*10^{-3}s^{-1} * [N2O5]

Part B

Replacing the value of the concentration of N2O5 given, we can get the rate of reaction:

rate= 4.82*10^{-3}s^{-1} *2.80*10^{-2}M

rate= 1.35*10^{-4}Ms^{-1}

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