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Chapter 8: Problem 83

Would you expect a reaction in which all reactants are in the gas phase to go faster, slower, or remain at the same rate if the temperature is increased while everything else is held constant? Explain your answer.

Short Answer

Expert verified
In conclusion, we would expect a reaction with all reactants in the gas phase to go faster when the temperature is increased, while everything else is held constant. This is due to the increased kinetic energy of the molecules, leading to more effective collisions that can overcome the activation energy barrier, as explained by the Arrhenius equation and collision theory.

Step by step solution

01

Collision Theory

Collision theory states that for a reaction to occur, reactant molecules must collide with proper orientation and with sufficient energy to overcome the energy barrier (activation energy).
02

The Arrhenius Equation

The Arrhenius equation relates the rate constant (k) of a reaction to its activation energy (Ea) and temperature (T): \[k = Ae^{\frac{-Ea}{RT}}\] where: - k is the rate constant - A is the frequency factor or pre-exponential factor - Ea is the activation energy - R is the gas constant - T is the temperature in Kelvin
03

Effect of Temperature on Reaction Rate

According to the Arrhenius equation, when the temperature increases, the exponent \(\frac{-Ea}{RT}\) becomes less negative, resulting in an increase in the rate constant (k). This in turn leads to an increased reaction rate. This can be explained through collision theory as well. When the temperature increases, the molecules have more kinetic energy, which leads to a higher chance of collisions with the required energy to overcome the activation energy barrier. So more molecules can collide with proper orientation and sufficient energy, which increases the reaction rate.
04

Conclusion

If the temperature is increased while everything else is held constant, we would expect a reaction with all reactants in the gas phase to proceed at a faster rate. This is due to the increased movement and kinetic energy of the molecules, leading to more effective collisions that are energetic enough to overcome the activation energy barrier.

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