Formula of Magnesium Oxide
Chemistry Practical Assessment: Finding the formula of Magnesium Oxide (Skill 3) Results: Table showing measurements before experiment: Mass of crucible (g) Mass of lid (g) Mass of magnesium (g) Mass of crucible and magnesium (g) st try 4.21 1.91 0.9 5.11 2nd try 4.23 1.91 0.9 5.13 3rd try 4.21 1.92 0.8 5.11 Average 4.21 1.91 0.9 5.11 Table showing measurements after experiment: Mass of crucible (g) Mass of lid (g) Mass of contents (g) Mass of crucible and contents (g) st try 4.21 1.91 0.07 5.18 2nd try 4.23 1.91 0.06 5.19 3rd try 4.21 1.92 0.05 5.16 Average 4.21 1.91 0.06 5.18 Mass of products and reactants: ? mass of crucible: 14.21g ? mass of crucible and magnesium before heating: 15.11g ? mass of crucible and magnesium after heating: 15.18g ? mass of magnesium before heating: 0.90g ? mass of magnesium oxide: 0.97g ? mass of oxygen: 0.07g Changes occurring during the reaction: • Magnesium stripe glowed and burned bright orange • Sparks appeared on the surface of the magnesium stripe • Started to shrink and change into white powder form but still glowing This shows that magnesium has reacted with oxygen to form magnesium oxide, a white powder. Appearance of contents at the end of experiment: • White powder • Not in a shape of a coil Number of moles of magnesium and oxygen in magnesium oxide:
displacement reactions of metal
Lab Report on Displacement Reactions of Metals * Hypothesis I can predict that a more reactive metal will displace a less reactive metal from its salts. To predict the displacement, I have applied the knowledge of reactivity and this is my prediction: Copper Magnesium Iron Zinc Magnesium Iron Zinc Copper Magnesium will displace zinc, iron and copper as it is a very reactive metal. Zinc will displace iron and copper but not magnesium as magnesium is more reactive. Iron will displace copper only as it is a less reactive metal. And copper will not be able to displace any metals because it is a very weak metal. * Method 1. I had placed the three pieces of the four different metals on a tile containing twelve holes. 2. Then I added the aqueous solution that is magnesium solution, iron solution, zinc solution & copper solution onto the different metals. 3. Then the reaction took place and I noted the results and the observations. * Results & Observations Metals + Aqueous solutions Results . Copper + Magnesium sulphate No reactions 2. Copper + Iron sulphate No reactions 3. Copper + Zinc sulphate No reactions . Magnesium + Iron sulphate Bubbles were formed, it had
Rate of Reaction Lab
Rates Of Reactions: Lab Report Introduction: In chemistry recently we have been doing the topic of Reactions. In this topic we have been learning about why elements react, how they react and what affects the reaction. For instance, temperature affects the speed of a reaction, and sometimes if there is any reaction at all. Aim: The aim of my experiment is to see how the factor of surface area affects the speed (rate) of a reaction between Hydrochloric Acid and Calcium Carbonate. Hypothesis: I know that the greater the surface area, the faster the reaction. Hence I predict that when I react Hydrochloric Acid with Calcium Carbonate, the Calcium Carbonate marbles will react slower than the Calcium Carbonate powder, as I think the powder has a higher surface area. The variables are as follows: Independent Variable: I shall be changing the surface area of the Calcium Carbonate to prove or disprove that it actually makes a difference to the rate of reaction. Dependant Variable: The Carbon Dioxide given off will be my dependant variable in this experiment. Control: I shall try to control the amount of Calcium Carbonate and acid in each experiment, so it is as close to being the same as possible. Apparatus: -Beaker -Measuring Cylinder -Calcium Carbonate -Scales -Hydrochloric Acid (0.4M) -Pipette Diagram: Method: The apparatus was gathered and set up.
In my investigation I am going to look at how concentration affects the rate of reaction, and the reaction I am going to look at is Sodium Thiosulphate (Na2 S2 O3) and Hydrochloric Acid (HCl).
An Investigation into the rate of reaction is affected by the concentration of a solution The rate of a reaction is the speed at which the reactants change into products. Reactions can be fast and slow for example rusting is a slow reaction and magnesium reacting with oxygen is an example of a fast reaction. There are several factors that affect the rate of reaction these include - ==> Surface area/size of solid particles ==> Concentration of solutions ==> Temperature ==> Presence of a catalyst Aim In my investigation I am going to look at how concentration affects the rate of reaction, and the reaction I am going to look at is Sodium Thiosulphate (Na2 S2 O3) and Hydrochloric Acid (HCl). The equation for the experiment is shown below - Na2 S2 O3 (aq) + 2HCl (aq) 2NaCl (aq) + S (s) + SO2 (g) + H2O (l) In previous times seeing this experiment I have seen what happens, the solution (which is made up of Sodium Thiosulphate and Hydrochloric acid) has become cloudy, this is because the sulphur is precipitated and sulphur is insoluble. In my experiment I am going to time how quickly it takes the solutions of different concentrations to produce solid sulphur, observing how quickly an "X" is observed under a conical flask of solution. When the "X" is obscured the reaction has went to the same point. Prediction I predict that the stronger concentration of sodium
In this investigation we are going to measure the rate of reaction of marble and HCl when the concentration or surface area of marble is changed.
Chemistry Coursework-Investigation on the rate of reaction between HCl (Hydrochloric acid) and Marble (Calcium Carbonate - CaCO3) Aim: In this investigation we are going to measure the rate of reaction of marble and HCl when the concentration or surface area of marble is changed. Introduction: A rate of reaction is the speed at which reactants become an end product. For a reaction to happen, the particles that are reacting have to collide. If they collide, with enough energy and pressure, then they will react. There are several factors that affect the rate of reaction. Firstly temperature will affect the rate of reaction; if the temperature is cold the particles will move more slowly, with less energy resulting in a slower reaction. However in a hot temperature the particles move more quickly, they collide more with more energy, creating a faster rate of reaction. Secondly concentration will affect it, the lower the concentration the more spread out the particles, so they will collide less and create a slower rate of reaction. Thirdly using a catalyst can be used to speed up a reaction, without it being changed. The factor that we will be investigating is the size and surface area, large particles have a small surface area so there are less particles exposed for collision, which means a slower reaction. However small particles have larger surface area and have faster
I measured the effect of concentration on the rate of reaction. The reactants were Sodium thiosulphate and Hydrochloric acid.
Data Analysis - Chemistry Coursework The effect of concentration on the rate of reaction ANALYSIS: For my data analysis, I measured the effect of concentration on the rate of reaction. The reactants were Sodium thiosulphate and Hydrochloric acid. This reaction made the products sodium chloride, sulphur dioxide, sulphur and water. When an acid is added to sodium thiosulphate, a yellow, cloudy precipitate is formed. And, as the sodium thiosulphate becomes more and more diluted, the solution takes longer and longer to form. However, in order for the reaction to take place, the reactants must first collide with each other. The collision theory should take place with the minimum amount of energy; this is called the activation energy. Head on collisions contain more energy, if collisions have enough energy then the collision that took place is successful and therefore a reaction occurs, however this isn't the case with all collisions. The collisions happen regardless of whether both the particles are in the solution, or whether one is in the solution and the other is a solid. The chances of collision are higher when the concentration is higher. For many reactions that involve liquids or gases, the increase of concentration on the reactants will increase the rate at which the reaction takes place. The point at which the reaction starts is called the energy barrier. When this
Rates of Reaction Practial
Rates of Reaction Practical Aim: The aim of this investigation is to investigate how the rate of reaction of Calcium Carbonate (CaCO3) with Hydrochloric acid (HCl) could be affected by surface area. Equation: HCl(aq) + CaCO3(s) CaCl2(aq) + CO2(g) + H2O(l) Hypothesis: I predict that the more the surface area the faster the rate of reaction because it increases the chances of collision. This is because more calcium carbonate is exposed to the acid molecules so they are more likely to collide. When measured in the same mass the smaller chips have a larger surface area altogether. Here is a diagram to show this: (if cut into 8 equal pieces) ==> Apparatus: - Two beakers (400ml) - Large Calcium Carbonate Chips (5g) - Small Calcium Carbonate Chips (5g) - Calcium Carbonate Powder (5g) - Hydrochloric Acid 1M (100ml) - Spatula - Accurate Scale - Stopwatch Method: . Collect all of the equipment and measure 5g of each size of surface area of Calcium Carbonate with a spatula. 2. Collect 100 ml of Hydrochloric Acid into one of the 400ml beakers. 3. Place the other beaker on the scale and then set the scale measure to zero. Pour the 100ml of HCl into the beaker on the scale. 4. Hold a stopwatch in one hand, and place the
The effects of concentration on reaction rates
John Saunders (11R) The effects of concentration on the rate of reaction between magnesium (Mg) and Hydrochloric acid (HCl). Introduction: In this experiment, I am going to find out what happens when different concentrations of hydrochloric acid are mixed with the same amounts of magnesium. The probable outcome of this is that the reaction will be more vigorous to start with, meaning the reaction would end up being completed faster, if the concentration was to be higher than normal. This would happen because there would be more atoms of hydrogen and chlorine in a higher concentrated solution, to react with the magnesium. As you can see, the circles that represent the hydrogen and chlorine atoms of the hydrochloric acid find it a lot harder to fit inside the right-hand rectangle, that is the same area as the left rectangle (the rectangles representing the solution of acid). This means that the right-hand rectangle is more concentrated, as the hydrogen and chlorine atoms take up more space. If a piece of magnesium were to be placed in the rectangles, then the more vigorous (and faster) reaction would take place in the right-hand rectangle. This is because the magnesium would be confined to the (smaller) area where there aren't hydrogen or chlorine atoms, so the collision rate is likely to be higher. Prediction: I predict that the higher the concentration of HCl, the
How the Concentration of Acid in a Solution affects the Rate of Reaction
Investigation into: How the Concentration of Hydrochloric Acid in a Solution affects the Rate of Reaction Aim: This experiment was to observe how the concentration affects the rate of reaction between chemicals. The two chemicals used in our experiment were Sodium Thiosulphate and Hydrochloric Acid. Introduction: The rate of reaction is basically the speed of how fast the reaction occurs between two reactants. You measure this speed in seconds, and have to set an achieving limit, which is a standard point of the reaction where a change is noticed and that is where the time must be recorded. A reaction is the simply the collision of the particles in two different substances (reactants). This essay is about writing how we observed the chemical reaction we carried out. Now here's the bit where the story gets interesting... My Prediction: My prediction is that: as long as the chemicals react in the same amount as was set, the speed of the reaction will be faster as the concentration (molarity) of the Hydrochloric Acid is increased. I predicted this because generally, when something has a higher concentration, it reacts quicker than when it has a lower concentration. This theory is ~ "Increasing the concentration increases the rate of reaction". This is because when there are more particles present, there is more collision between the particles; this increases the rate of
Rates of reaction of agar with different HCL concentrations
Rates of Reaction Background Info Collision Theory Different reactions can happen at different rates. The rate of the reaction tells us how quickly a chemical reaction happens. Reactions that occur slowly have a low rate of reaction. Reactions that happen quickly have a high rate of reaction. For example, rusting is a slow reaction: it has a low rate of reaction. Burning and explosions are very fast reactions: they have a high rate of reaction. For a chemical reaction to occur, the reactant particles must collide. But collisions with too little energy do not produce a reaction. The particles must have enough energy to overcome the activation energy in order for the collision to be successful in producing a reaction. Activation energy is the energy needed to start a reaction. The rate of reaction depends on the rate of successful collisions between reactant particles. The more successful collisions there are, the faster the rate of reaction. There are two ways to find the rate of a reaction: * Measure the rate at which a reactant is used up * Measure the rate at which a product is formed The method chosen depends on the reaction being studied. Sometimes it is easier to measure the change in the amount of a reactant that has been used up; other times it is easier to measure the change in the amount of a product that has been produced. Reactions where a single species
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