Rate constants for the reaction NO2(g)+CO(g) →NO(g)+CO2(g) are 1.3 M^-1 s^-1 at 700 K and 23.0 M

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Rate constants for the reaction NO2(g)+CO(g) →NO(g)+CO2(g)...

Rate constants for the reaction $\mathrm{NO}_{2}(g)+\mathrm{CO}(g) \rightarrow$ $\mathrm{NO}(g)+\mathrm{CO}_{2}(g)$ are 1.3 $\mathrm{M}^{-1} \mathrm{s}^{-1}$ at 700 $\mathrm{K}$ and 23.0 $\mathrm{M}^{-1} \mathrm{s}^{-1}$ at 800 $\mathrm{K}$ (a) What is the value of the activation energy in $\mathrm{kJ} / \mathrm{mol}$ ? (b) What is the rate constant at 750 $\mathrm{K}$ ?

Rate constants for the reaction $\mathrm{NO}_{2}(g)+\mathrm{CO}(g) \rightarrow$
$\mathrm{NO}(g)+\mathrm{CO}_{2}(g)$ are 1.3 $\mathrm{M}^{-1} \mathrm{s}^{-1}$ at 700 $\mathrm{K}$ and 23.0 $\mathrm{M}^{-1} \mathrm{s}^{-1}$ at 800 $\mathrm{K}$
(a) What is the value of the activation energy in $\mathrm{kJ} / \mathrm{mol}$ ?
(b) What is the rate constant at 750 $\mathrm{K}$ ?

Key Concepts

Arrhenius Equation

The Arrhenius equation is a fundamental expression in chemical kinetics that relates the rate constant of a reaction to temperature and activation energy. Its exponential form, k = A exp(?Ea/(RT)), allows one to analyze how changes in temperature affect the reaction rate and to extract the activation energy from experimental data.

Activation Energy

Activation energy is the minimum energy barrier that reactant molecules must overcome in order to transform into products. It is a crucial parameter in determining the temperature dependence of reaction rates, with higher activation energies generally leading to slower reactions at a given temperature.

Rate Constant

The rate constant is a proportionality constant in the rate law equation of a chemical reaction, providing a measure of the reaction's speed under specified conditions. It encapsulates the effects of both the collision frequency between molecules and the probability that collisions will result in a reaction.

Temperature Dependence of Reaction Rates

Temperature significantly influences the rate of chemical reactions. According to the Arrhenius equation, an increase in temperature leads to an increase in the rate constant, because a larger fraction of molecules have enough kinetic energy to overcome the activation energy barrier, resulting in faster reaction rates.

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