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28 Nov 2019

Consider the second-order reaction:

2NO2(g)?2NO(g)+O2(g)

Use the simulation to find the initial concentration [NO2]0 and the rate constant k for the reaction. What will be the concentration of NO2 after t = 40.0s
([NO2]t) for a reaction starting under the condition in the simulation?

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Jamar Ferry
Jamar FerryLv2
22 Nov 2019

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Related questions

1) The rate of reaction in terms of the "rate law expression" includes the rate constant (k), the concentration of the reactants, and the orders of the reaction with respect to the different reactants.

Consider the following reaction:

A+B→C+D

The initial concentrations of the reactants A and B are 0.380 M and 0.320 M, respectively.

The rate of reaction is 0.060 M⋠s−1, and the orders of the reaction, with respect to reactants Aand B, are 1 and 2, respectively.

Determine the rate constant (k) for the reaction using the rate law.

Express your answer in M−2⋠s−1 to three significant figures.

2)

consider the second-order reaction:

2HI(g)→H2(g)+I2(g)

Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction. What will be the concentration of HI after t = 3.07×1010 s ([HI]t) for a reaction starting under the condition in the simulation?

Express your answer in moles per liters to three significant figures.

The gas-phase decomposition of NO2, 2 NO2(g) 2 NO(g) + O2(g), is studied at 383 °C, giving the following data:

(a) Is the reaction first order or second order with respect to the concentration of NO2? (b) What is the rate constant? (c) Predict the reaction rates at the beginning of the reaction for initial concentrations of 0.200 M, 0.100 M, and 0.050 M NO2.

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