Kinetic Energy is the energy of movement, whether it is horizontal or vertical, it’s kinetic. There is many different types of kinetic energy. There is; vibrational, rotational and translational (the movement from one location to another. IN our experiment we also have kinetic energy. The particles that move around need kinetic energy to bond because if the particles wouldn’t have kinetic energy, they wouldn’t move, then they wouldn’t be able to collide and at last there would be no chemical reaction taking place. But for a reaction to take place there has to be enough kinetic energy to overcome the bonding forces of the reactants. The minimum amount of kinetic energy need to cause a chemical reaction is called activation energy (symbol: Ea
The graph shows a linear relationship between light intensity between 0-150 µmoles photons m-2s-1 until the rate of oxygen production slowed between 150-350
In reference to the collision theory, molecules act as small spheres that collide and bounce off each other, transferring energy among themselves when the collide. In order for a reaction to occur, there must be collisions between molecules. Through experimentation, factors are discovered that influence the reaction rates of chemical reactions include the concentration of reactants, temperature, surface area, the physical state of reactants, and a catalyst. This experiment regarding the factors that affect reaction rate tests the effects of increased concentration and
A physical change includes a change in the material without affecting its composition, such as the physical state change. However, a chemical change includes the change in the composition of the substance. The change in color, formation of a gas or a solid product, and the production of energy are the evidences of a chemical reaction, thus, of a chemical change.
reaction has taken place, for example a gad is given off or a solid is
Abstract: This two part experiment is designed to determine the rate law of the following reaction, 2I-(aq) + H2O2(aq) + 2H+I2(aq) + 2H2O(L), and to then determine if a change in temperature has an effect on that rate of this reaction. It was found that the reaction rate=k[I-]^1[H2O2+]^1, and the experimental activation energy is 60.62 KJ/mol.
A chemical reaction is a process that involves change of the molecular or ionic structure of a substance, as opposed to a change in physical form or a nuclear reaction. The key concepts of a chemical reaction are:
It was researched that the greater the surface area of a solid, the faster the reaction rate. The collision theory states that the given reactants of a chemical reaction must successfully
In chemical reactions bonds must be broken and new bonds must be formed. In order for this to occur the bonds must be made less stable. For bonds to become less stable a small input of energy is required and this is
As told at the beginning of this lab report, our aim of this experiment was to test the validity of Hess’s law which suggests that the enthalpy change of a reaction must be equal to the sum of the enthalpy changes of the other reactions that relate to the original reaction. Our result achieved from this experiment is the simple proof of Hess’s Law’s validity.
There were errors involved and the calculations don’t seem 100% correct. Activation energy should have units of Joules only but when calculated the activation energy, it had units of Joules per moles times seconds. There was probably and error in the calculations or possibly just missing a step. There were also errors when recording time as the lab manual was not followed correctly. Assuming that all experiments that took place were 1st order reactions doesn’t seem correct. R2 was higher compared to the 0th order but only barely and I was unable to determine which was the correct order of the reaction. The results seem to make sense in terms of activation energy. As temperature is being increased more heat is being released and thus activation energy is lower at higher temperatures. There’s not a huge difference in temperature but there’s a slight difference in temperature which causes the slight difference in activation