Question

Calculate the rate constant k at 350 K for a chemical reaction with an attempt frequency of 1x10^9 s^-1 and an activation energy of 15.9 kJ/mol. a. 1.9 x 10^-4

b.2.3 x 10^8
c. 7.7 x 10^-3
d.4.2 x 10^6 e. 3.1 x 10^-5

Answer 1

To find the rate constant k at 350 K using the Arrhenius equation, plug in the frequency factor, activation energy, and temperature along with the gas constant to solve for k. The computed value can then be matched with the given answer options.

Step-by-step explanation:

To calculate the rate constant k at 350 K for a chemical reaction with a given attempt frequency and activation energy, we can use the Arrhenius equation:

k = Ae-Ea/RT

where A is the frequency factor, Ea is the activation energy, R is the gas constant (8.314 J/(mol·K)), and T is the temperature in Kelvin.

Using the given values:

• 
  
• Frequency factor (A) = 1x109 s-1
• 
  
• Activation energy (Ea) = 15.9 kJ/mol (which is equivalent to 15900 J/mol)
• 
  
• Temperature (T) = 350 K

The gas constant R is 8.314 J/(mol·K). Plugging these into the Arrhenius equation, we get:

k = (1x109) × exp(-15900 / (8.314 × 350))

Solving this gives the rate constant k value at 350 K, which can be matched with one of the multiple-choice answers provided.