The effect of concentration on the rate of reaction between magnesium and acid! Aim – To investigate how concentration effects the rate of reaction between magnesium and hydrochloric acid. Prediction – I predict that the weaker the hydrochloric acid is the slower the gas will collect. This is because in a weaker concentrated solution there is less acid molecules to react with magnesium. This is to do with the kinetic theory. Background information on reactions – The kinetic theory is in solutions of higher concentration and in gases at higher pressure, particles are closer together. They have a greater chance of colliding, because there are more collisions the reaction rate is greater.
Increasing the concentration of reactants increases the rate of a reaction. This is because there are more particles in the same volume so more collisions are possible every second. For a chemical reaction to take place, some bonds in the reactants must be broken. The colliding particles must have enough energy to break these bonds. This minimum amount of energy is called the activation energy. Only the particles moving very fast have enough energy to break bonds.
In gases, liquids and in solution, the particles move at a range of speeds. Some are moving very slowly and others are moving very fast. To react, particles must collide with enough energy and in the correct orientation for bonds to be broken. Safety precautions – Were safety goggles at all times during the experiment. Beware of spilling the hydrochloric acid. Making it a fair test – Keep the temperature of the acid the same at all times.
The Coursework on Grams Of Limestone Acid Particles Reaction
Aim In this investigation I am aiming to find out how the concentration of acid affects the rate of reaction with Calcium Carbonate (Limestone). Hypothesis I predict that the higher the concentration of acid then the faster the rate of reaction. Calcium Carbonate + Hydrochloric Acid = > Carbon Dioxide + Calcium Chloride CaCO 3 + 2 HCl = > CO 2 + H 2 O + CaCl 2 I predict this because when a ...
Get the acid from the same bottle every time to make sure it is the same concentration. Any result I find slightly strange or different I will double check. I will repeat the whole experiment twice to make sure i have it all correct. Equipment – safety goggles 100 ml Conical flask 100 cm 2 gas syringe instead of using beehive funnel and delivery tube Two 25 ml measuring cylinders Hydrochloric acid Water Stop watch Diagram – Method – I will fill up a 100 ml conical flask with 25 mls of hydrochloric acid. I will then add 10 cm of magnesium ribbon instead of 5 cm as the reaction was not strong enough to measure.
Then I’ll connect the gas syringe using the stopper to begin the experiment. I’ll then take a stop watch and take the time down for every 10 cm 2, and stop timing when the syringe fills to 100 cm 2. I will then start all over again but instead of beginning with 25 mls of hydrochloric acid on it’s own, I will continue as in the table below! Then repeat the experiment. Results – Conclusion – Over all I think my decision to change the way in which I go around doing the experiment was a good idea. Using the beehive funnel and delivery tube was just a complicated way of doing what I finally did. I believe my experiments went well and I got fairly good results.
In my prediction I wrote. “I predict that the weaker the hydrochloric acid is the slower the gas will collect. This is because in a weaker concentrated solution there is less acid molecules to react with magnesium.” My prediction was correct and it was extremely noticeable, as you will notice in my results.
