REFERENCES GENERAL CHEMISTRY FOR ENGINEERING AND SCIENCE II CHE 152-50 Factors Which Influence the Rates of Reactions pages 1-10 OBJECTIVES To examine the factors which cause the rate of chemical reactions to change. QUESTION The question that was proposed for investigation was: Do all factors change the rate equally? Background Discussion For this experiment you have to have a basic understanding of Collision Theory to understand what’s going on in the experiment. Collision Theory is a model of chemical reactions in which a reaction occurs after a collision containing enough energy occurs between two reactant molecules. This model has five factors which can be affected and they are the nature of reactants, temperature, concentrations, surface area and catalyst. If one of these were changed then the reaction could occur faster or slower depending on what was changed. Sample Calculations Rate Law: 2A + B→C,is rate=k[A][B] (Lab Guide pg.6) PROCEDURE (Attached) DATA TABLES/CALCULATIONS (Attached) RESULTS HYPOTHESIS All factors change the rate of reaction equally. OBSERVATIONS In this experiment there five different phases and in each a different factor of the Collision Theory was tested. The first phase was called, Nature of the Reactants and it had three parts to it. In the first part of it which was steps 1-4, 5 pieces of mossy zinc were put into 3ml of 2M H_2 〖SO〗_4 and during this time bubbles were produced. After a few minutes the zinc was removed from the acid and it was now clean zinc. In the second part of phase 1 which was steps 5-8 4 different pieces of clean zinc were placed in 4 different acids. The acids were Hydrochloric ... ... middle of paper ... ...e will also become faster. In phase one, Nature of the Reactants five different metals were placed in the 2M HCl they all reacted differently with magnesium being the most reactive and copper being the least reactive. In phase two, Concentration, zinc was placed in different concentrations of 6M HCl. The higher the concentration was the more reactive the metal was. Next in phase three, Temperature, zinc was added to 6M HCl which was a different temperatures and the zinc was the most reactive with the HCl in the boiling water and least reactive with the HCl in the ice bath. Then in phase four, Surface Area, the powered zinc was more reactive then the piece of zinc in the 6M HCl because it had more surface area to be covered than the piece of zinc. Lastly in phase 5, Catalyst, the 3% H_2 O_2 was reactive with the 5 drops of 〖FeCl〗_3 but not with the 5 drops of water.
Investigation of the reaction between hydrochloric acid and marble chips A chemical reaction is when two or more substance called reactants are chemically bonded to form a new product, as a result of the process, for a reaction to take place, the particles must have enough kinetic energy to collide and form new bonds , this is called a successful collision. The minimum amount of energy needed for a successful collision is activation energy, which is “The energy that an atomic system must acquire before a process can occur”. Chemical reaction is different to a physical reaction, chemical reaction are not reversible and results in a new product, however a physical reaction can be easily reversed as it only changed its state. The activation energy is able to loosen particles and enable them to from new bonds to produce new products. The faster the molecules are moving the bigger the chance of a successful collision, so the faster and stronger the reaction will be , the more kinetic energy a reactant has the easier it is for the new bonds the collide and produce new bonds.
3. Drop tablet of Alka-Seltzer into the cold beaker of water and time length of reaction with a stopwatch
The purpose of the experiment is to study the rate of reaction through varying of concentrations of a catalyst or temperatures with a constant pH, and through the data obtained the rate law, constants, and activation energies can be experimentally determined. The rate law determines how the speed of a reaction occurs thus allowing the study of the overall mechanism formation in reactions. In the general form of the rate law it is A + B C or r=k[A]x[B]y. The rate of reaction can be affected by the concentration such as A and B in the previous equation, order of reactions, and the rate constant with each species in an overall chemical reaction. As a result, the rate law must be determined experimentally. In general, in a multi-step reac...
However, only experiments IV “Effect of Copper Metal” and V “Effect of Temperature” had reasonable results, so copper metal and temperature are the more effective factors. The less effective factors are the changes in concentrations of "H" ^"+" ions and "C" _"2" "O" _"4" "H" _"2" particles. This observation is represented in experiments II “Effect of "H" ^"+ " Ions” and III “Effect of "C" _"2" "O" _"4" "H" _"2" Concentration.” Both runs 2B and 2C had the fastest times of 25 seconds and 86 seconds
It is important however to note that the NH4 and K ions are still in
For this experiment we have to use physical methods to separate the reaction mixture from the liquid. The physical methods that were used are filtration and evaporation. Filtration is the separation of a solid from a liquid by passing the liquid through a porous material, such as filter paper. Evaporation is when you place the residue and the damp filter paper into a drying oven to draw moisture from it by heating it and leaving only the dry solid portion behind (Lab Guide pg. 33.).
The purpose of the lab was to show the effect of temperature on the rate of
Input variables In this experiment there are two main factors that can affect the rate of the reaction. These key factors can change the rate of the reaction by either increasing it or decreasing it. These were considered and controlled so that they did not disrupt the success of the experiment. Temperature-
The aim of this experiment was to investigate the affect of the use of a catalyst and temperature on the rate of reaction while keeping all the other factors that affect the reaction rate constant.
The fourth factor is to add a catalyst, but in this experiment we did not add a catalyst. Knowing the collision theory, it makes my predictions clearer with what is going to happen when the experiment will take place.
The faster the cross disappears the faster the reaction and by timing how long this takes, we can establish the rate. of the reaction of the. I predict that the greater the concentration of sodium thiosulphate. solution in the experiment, the faster the chemical reaction will take. place. The sand is a sand.
3.0g of salicylic acid was weighed (salicylic acid was formed from Step 1) into a 100mL beaker. In a 10mL graduated cylinder, 5.0mL of acetic anhydride was measured and was transferred into the 100mL beaker. 5 drops of concentrated sulphuric acid was also added into the beaker.
This experiment deals with motion. This study of motion is called Kinematics. Kinematics studies the possible motions. (http://www.britannica.com/EBchecked/topic/318099/kinematics). Kinematics is used to show the displacement of an object, the rate an object is moving (velocity), and the change in velocity (acceleration). This is graphed against time individually to determine if the motion is uniform or nonuniform and if the acceleration is uniform or nonuniform. Uniform motion is when an object has a constant speed and direction. Nonuniform motion is when there is either a change in speed or a change in direction. When the graphing has completed, other properties can be discovered like the instantaneous velocity. Instantaneous velocity is used to present the velocity of an object in a specific time when the velocity is changing. Vector and scalar quantities are also very important in this experiment.
In chemistry, catalyst is a substance which increases the rate of reaction with itself does not combine in reaction. The aim of this essay is researching more about catalyst, for instant how does catalyst work and the example of catalyst. Also, this research might useful for science international foundation students for support revision. First of all, this essay will describe Maxwell Boltzmann distribution diagram and give the meaning of collision theory, then it will discuss on Activation Energy. After that, activation complex will be explained using enthalpy diagram and catalyst pathway will be focused. Following this, there will be a describing about homogeneous and heterogeneous catalysts, also their own mechanisms and examples. Lastly, this essay will represent the catalytically poisoning.
There are five factors which affect the rate of a reaction, according to the collision theory of reacting particles: temperature, concentration (of solution), pressure (in gases), surface area (of solid reactants), and catalysts. I have chosen to investigate the effect of concentration on the rate of reaction. This is because it is the most practical way to investigate. Dealing with temperatures is a difficult task, especially when we have to keep constant high temperatures. Secondly, the rate equation and the constant k changes when the temperature of the reaction changes.