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I m doing an experiment between acids and marble chips there are many different ways to do this type of experiment
Reaction rate is affected by these four things
The collision theory relates molecule collisions to reaction rate.
According to this theory, reacting molecules must collide with sufficient energy if they are to form products
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· Surface area when one of the reactants is a solid, the reaction can only take place at the surface of the solid. Breaking the solid into smaller pieces will increase the surface area exposed to the other reactant. This should increases the reaction rate.
· Temperature since temperature is a measure of the motion of particels, increasing the temperature will cause the particles to move faster. When particles move faster, more collisions occur and the collisions are more violent. This should increase the reaction rate.
· Catalysts catalysts are substances that change the rate of a chemical reaction without being changed in the reaction. Catalysts are most often used to speed up a chemical reaction. They do this by changing the steps needed between the reactants and the formation of the products. If the number of steps can be reduced, the reaction rate should increase.
There are types of reactions
Exothermic reaction - a reaction that releases energy. The reactants have more energy than the products. Energy must be released as the products form. The container in which an exothermic reaction is taking place will feel hot.
Endothermic reaction - a reaction that absorbs energy. The products have more energy than the reactants. Energy must be absorbed as the products form. The container in which an endothermic reaction is taking place will feel cold
Paul Leslie 11h
Plan
I want to make sure my experiment is fair so I m going to make sure that I m using the same about every time I do the experiment like use 0 cm of acids each time use 10 g of marble chips each time as well
1) put 10 g of marble chips into a conical flask
) add 0cm of 0.5 hydrochloric acid into the flask Immediately connect the syringes and start the stop clock
) take the reading on the syringes every 10 sec for about min
4) wash out the flask and then do the experiment again using 1 m of acid and 10g of marble chips
5) repeat the experiment using 1.5m and .0m of hydrochloric acid
Prediction
If the reaction between marble chips and acids is going to take place, the marble ions in the acid must come in contact with acids ions. If the concentration of the acid is increased the number of ions smoking about in 1 cm the solution will increase and there will there fore be an increase in the number of collisions with the marble.
How ever not all of these collisions will lead to chemical reaction since some of the particles will not have enough energy to collide the more the chemical reaction will take place
This mean that the rate of an chemical react will increase if the concentration of reactants is increase if the concentration of reactions is decreased the rate of the chemical reaction will decrease.
Rates of reaction
How fast a reaction can occur?
E.g. Fast Fireworks slow rusting
Explosive
Rates are a measure of something changing over time
Temperature
Gas given off
Color change
PH
Concentration
Mass
Choosing something that changes over time. This can be done by looking at the equation.
Choosing a variable to change over time and then plot a graph.
Factors that Effect Rates of Reactions
Concentration
Concentration appears in many guises. For example, pressure and surface area (or state of subdivision) are really both concentration terms. As the concentration increases chemical reaction rates increase. The difference between iron slowly rusting in a field and a fourth of July sparkler (which is just powdered iron reacting with air) is the surface area of the iron (and, of course the temperature of the sparkler). We might argue that proofing yeast by adding a little sugar to the yeast before making bread is an increase in concentration causing an increase in the rate of the yeast metabolism. Im somewhat amused to admit that there are relatively few common examples of this effect.
Nature of the reactants
This is another way of saying that different chemicals may react at different rates even though the overall chemistry may look the same. A simple example is that lithium, sodium, potassium and cesium all react with water to give hydrogen. Lithium reacts somewhat slowly and is unexciting. Sodium reacts quickly, skimming along the surface of the water on a layer of hydrogen. If the sodium piece gets stuck on the wall of a container the temperature may rise enough for the hydrogen to be ignited. Potassium reacts so vigorously with water that the hydrogen bursts into flame with the oxygen in the air, while cesium effectively explodes when it hits water.
Paul Leslie 11h
Catalyst
Catalysts are materials that increase the rates of chemical reactions although they are not used up in these reactions. Catalysts operate by either altering the pathway of the reaction (mechanism) or by altering the effectiveness of the interaction between two compounds by serving as a template for the compounds. The classic catalyst that everyone knows is the catalytic converter in the exhaust line of a car, which acts to burn residual hydrocarbons to carbon dioxide and water.
Summary
These factors that affect reaction rates may easily be understood if we understand the simple principles that must take place if a chemical reaction is to occur.
Paul Leslie 11h
The results
time every 10 sec .0M .0M .0M average
10 15 15 16 16
0 5 5
0 48 48 57 5
40 68 68 8 7
50 85 85 100 1
60 100 100
70
80
0
100
time every 10 sec 1.5M 1.5M 1.5M average
10 1 1 14 1
0 4 0 6
0 8 6 45 40
40 5 54 58 55
50 65 64 67 65
60 75 7 85 7
70 85 80 4 86
80 88 over 100 0
0 over 100 6 6
100 over 100
time every 10 sec 1.0m 1.0m 1.0m average
10 10 1 8 10
0 0 18 0
0 0 8 0
40 4 4 7 40
50 5 50 46 50
60 68 58 54 60
70 80 67 64 70
80 0 74 7 78
0 8 80 87
100 over 100 0 87 8
time every 10 sec 0.5M 0.5M 0.5M average
10 4 4
0 4 8 8 7
0 6 1 1 10
40 8 16 16 1
50 10 0 17
60 1 6 6 1
70 14 0 5
80 16 8 4
0 18 4 8
100 0 45 44 6
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