As the temperature is increased in a reaction, the reaction will proceed faster. This is due to the increased collisions of molecules within the solution that is undergoing the reaction. When the temperature is increased, the kinetic energy of the molecules is increased and causes more collisions to occur. This allows the reaction to occur faster. The activation energy is decreased when the temperature is increased. The activation energy is the minimum amount of energy to start a reaction. This is because the increased amount of collisions between molecules allows bonds to break easier and the reaction to proceed at a faster rate, requiring less energy for the reaction to start. According to the graph that was created with the data collected in experiment four (the natural log the the rate constant k, over the inverse of temperature in kelvin), the activation energy can be found through the slope of the graph. In this case, the slope is negative. This demonstrates that as the temperature is increased, it takes less energy required to start the reaction. The Arrhenius plot is an accurate way to solve for variables in the Arrhenius equation. Some possible variables one could solve for is the activation energy (slope equals the negative value of the activation energy divided by the gas rate constant) and the natural log of A (the y-intercept of the graph). The rate constant is increased as the temperature is increased. The rate constant is solved by dividing the rate of the reaction by the multiplication of both the concentrations of each solution used. Due to the fact that the rate had increased as the temperature was increased, the rate constant value increased as well. This is because the the rate was in the numerator of the rate constant equation. As the numerator got larger, so did the rate constant.