Magnesium metal in form of a ribbon or powder reacts with acids rapidly than water liberating hydrogen gas. These include the presence or absence of catalyst, temperature, concentration, and surface area of reactants. This could have increased or decreased the temperature of the HCl during the reaction.
These two theories justify the corresponding increase of both factors. Firstly, I will always wash out and replace the acid in the conical flask after every test to ensure there is no residue left and my results are as accurate as possible. Sometimes a 10 degree C temp. Once again, this can be avoided by performing the experiment in a closed room.
A catalyst is another substance which is not used up in the reaction and only speeds up the reaction, it does not cause more of the product to be produced.
Clean if necessary by rubbing lengths of the ribbon with fine sandpaper to remove the layer of oxidation. The measured duration of acid-metal reaction in seconds and the rate of gas bubbles.
There are four things that affect the rate of reaction between two substances usually a liquid and a solid. All the reaction will be carried out under a constant temperature room temperature of 25 0C. This could have been avoided by making a large amount of the HCl in the desired concentration at the beginning of the experiment.
These include the presence or absence of catalyst, temperature, concentration, and surface area of reactants. Rate of Reaction Graph 1 shows the relationship between change in temperature and the rate of reaction.
The rate of reaction at differing concentration is obtained by calculating the slope of time vs. The pressure of the test tube only during initial 70 seconds is measured to find the change in pressure.
I predict that the relationship between concentration and time is similar to that of inverse proportionality but it will not be identical.
Now, I will look at the effect of heat. The volumetric flask is capped and inverted several times.
Repeat steps 1 to 8 using 1M and 2M Hydrochloric Acid. Surface area of Magnesium ribbon: Pour the acid into the cm3 conical flask. Rate of reaction can be calculated by measuring the speed at which reactants are consumed or the speed at which products are formed. Furthermore, some reactions can be sped up depending on how much light they are exposed to.
Reactants with high surface area provide a greater binding surface for other reacting molecules, and therefore increase the number of successful collisions at any moment.The factors that may affect the rate of reaction are as follows: · Temperature of the Hydrochloric Acid · Mass of the magnesium ribbon used · Concentration of the Hydrochloric acid.
In a reaction between magnesium metal and hydrochloric acid, magnesium atoms must collide with the hydrogen ions. Consider the reaction between hydrochloric acid and zinc metal. In one beaker, Factors That Affect Reaction Rate ; pages Collision Theory and Concentration, Surface Area, Nature of Reactants, and.
- Investigating the Rate of Reaction Between Magnesium Ribbon and Hydrochloric Acid Aim: To find out the rate in which magnesium ribbon dissolves in different molars of hydrochloric acid, and which factors affect the rate of reaction.
The duration of reaction, (time taken for Magnesium to dissolve in hydrochloric acid completely) measured using a stopwatch in kaleiseminari.com rate of gas bubbles The independent variables Increasing concentration of hydrochloric acid: This will be changed by changing dilution kaleiseminari.come area of Magnesium ribbon: This will be changed by using Magnesium ribbons and powdered Magnesium.
Mar 24, · Effect of Concentration on the rate of reaction of magnesium ribbon in hydrochloric acid - High School Chemistry Guide In-text: (High School Chemistry Guide, ).
- Rate of Reaction Between Marble Chips and Hydrochloric Acid To investigate the factors which affect the rate of reaction between marble chips and hydrochloric acid, with one in specific detail.
Scientific knowledge: Marble chips erode when they .Download