The degradation of cf3ch2f (an hfc) by oh radicals in the troposphere is first order in each reactant and has a rate constant of k = 1.6 x 10^8 m^-1s^-1 at 4°c.
part a) if the tropospheric concentrations of oh and cf3ch2f are 8.1 x 10^5 and 6.3 x 10^8 molecules/cm^3, respectively, what is the rate of reaction at this temperature in m/s?

2.1 × 10⁻¹⁹ M/s

Explanation:

Let's consider the degradation of CF₃CH₂F by OH radicals.

CF₃CH₂F + OH → CF₃CHF + H₂O

Considering the order of reaction for each reactant is 1 and the rate constant is 1.6 × 10⁸ M⁻¹s⁻¹, the rate law is:

r = 1.6 × 10⁸ M⁻¹s⁻¹.[CF₃CH₂F].[OH]

where,

r is the rate of the reaction

If the tropospheric concentrations of OH and CF₃CH₂F are 8.1 × 10⁵ and 6.3 × 10⁸ molecules/cm³, respectively, what is the rate of reaction at this temperature in M/s?

The Avogadro's number is 6.02 × 10²³ molecules/mole.

The molar concentration of OH is:

The molar concentration of CF₃CH₂F is:

r = 1.6 × 10⁸ M⁻¹s⁻¹ × 1.0 × 10⁻¹² M × 1.3 × 10⁻¹⁵ M = 2.1 × 10⁻¹⁹ M/s

the right answer is c i just did the question.