The Dance of Molecules
Imagine a microscopic world inside a reaction vessel. Millions of gas molecules are constantly colliding, bouncing off each other in a chaotic dance. However, not every collision leads to a chemical reaction. For a reaction to occur, the colliding molecules must possess a certain minimum amount of kinetic energy, known as the activation energy (Ea).
If we plot the kinetic energies of all these molecules, we get the famous Maxwell-Boltzmann distribution curve. Most molecules have an average, moderate energy. Only a tiny fraction of elite molecules sit at the far right tail of the curve, possessing energy greater than Ea.
The Arrhenius Factor
Mathematically, this crucial fraction of molecules is given by the Arrhenius factor:
This elegant expression tells us exactly what portion of the total molecules is capable of reacting at a given absolute temperature T. Our goal in this problem is to calculate this fraction and compare it to the given expression e−x.
The Trap of Units
Before we plug in the numbers, we must be extremely careful with our units. This is a classic trap in physical chemistry! The activation energy is given as 80.9 kJ mol−1, but the universal gas constant R is given in Joules (8.31 J K−1 mol−1).
To ensure consistency, we must convert the activation energy into Joules by multiplying by 1000:
Ea=80.9×1000=80900 J mol−1
The Final Calculation
Now, let's substitute our values into the exponent term RTEa:
First, we multiply the terms in the denominator:
Next, we perform the division:
So, the fraction of molecules is approximately e−13.907. The problem states that this fraction is equal to e−x. Therefore, by comparing the exponents, we get:
Finally, the question asks us to round off the value of x to the nearest integer. Since 13.907 is much closer to 14 than to 13, we round it up.
Final Answer: