My Learning Cart
?
Categories
Account

For a reaction with an activation energy of 50 kJ/mol, what is the effect of inc

₹0.0
Login to Download
  • 📥 Instant PDF Download
  • ♾ Lifetime Access
  • 🛡 Secure & Original Content

What’s inside this PDF?

Question: For a reaction with an activation energy of 50 kJ/mol, what is the effect of increasing the temperature from 300 K to 350 K on the rate constant?

Options:

  1. Rate constant decreases
  2. Rate constant remains the same
  3. Rate constant increases
  4. Rate constant doubles

Correct Answer: Rate constant increases

Solution: 

According to the Arrhenius equation, an increase in temperature generally increases the rate constant due to the exponential dependence on temperature.

For a reaction with an activation energy of 50 kJ/mol, what is the effect of inc

Practice Questions

Q1
For a reaction with an activation energy of 50 kJ/mol, what is the effect of increasing the temperature from 300 K to 350 K on the rate constant?
  1. Rate constant decreases
  2. Rate constant remains the same
  3. Rate constant increases
  4. Rate constant doubles

Questions & Step-by-Step Solutions

For a reaction with an activation energy of 50 kJ/mol, what is the effect of increasing the temperature from 300 K to 350 K on the rate constant?
  • Step 1: Understand that the activation energy (Ea) is the energy needed for a reaction to occur. In this case, Ea is 50 kJ/mol.
  • Step 2: Know that temperature (T) is measured in Kelvin (K). We are increasing the temperature from 300 K to 350 K.
  • Step 3: Familiarize yourself with the Arrhenius equation, which is: k = A * e^(-Ea/(RT)), where k is the rate constant, A is the pre-exponential factor, R is the gas constant (8.314 J/(mol·K)), and T is the temperature in Kelvin.
  • Step 4: Recognize that as temperature (T) increases, the value of e^(-Ea/(RT)) increases because the exponent becomes less negative.
  • Step 5: Conclude that since the rate constant (k) is directly related to the exponential term, increasing the temperature from 300 K to 350 K will increase the rate constant.
  • Arrhenius Equation – The Arrhenius equation describes how the rate constant of a reaction depends on temperature and activation energy.
  • Activation Energy – Activation energy is the minimum energy required for a reaction to occur, influencing the rate constant.
  • Temperature Dependence – The rate constant increases with temperature due to the exponential factor in the Arrhenius equation.
Soulshift Feedback ×

On a scale of 0–10, how likely are you to recommend The Soulshift Academy?

Not likely Very likely
Home Practice Performance eBooks