Marble Chips and Hydrochloric Acid.

Marble Chips and Hydrochloric Acid PLANNING AIM To find if changing the concentration of an acid will increase or decrease the rate of the reaction when marble is dissolved in hydrochloric acid. With the equation CaCO3 + 2HCl CaCl2 +H2O + CO2 HYPOTHESES A reaction occurs when particles collide. This process is based on random particle movement. So therefore, the more particles you have in a space, the more likely they are to collide. Therefore making the reaction accelerate. This theory can be proved if you compare the rates of reaction with marble in hydrochloric acid. 'If the acid is of a higher concentration, the reaction will be quicker.' Also if the particles have more energy, they will be travelling faster, making them collide more frequently. PREDICTION When the concentration of acid increases, more gas will be given off faster. I know this from my trial experiments. METHOD Since I will be working with strong acid, I will wear safety goggles while conducting the experiment. I will use Marble chips all of a small size. I can use a sieve to make sure they are all roughly similar size- about 7mm diameter. The amount of acid I have decided on is 10ml. And so the amount of marble must be in excess - 3g. I can measure the speed of the reaction by how much gas is given off. I can measure this in cm3 in a gas syringe. when the experiment takes place, I will take

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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

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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

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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

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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

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My experiment will be conducted to find out at what concentration does sodium thiosulphate with hydrochloric acid have the most reaction and how the concentration generally affects the rate of reaction.

How does concentration affect rate of reaction? I am going to conduct an experiment on rate of reaction and how the concentration of sodium thiosulphate affects the rate of reaction. Several things such as temperature, ph and concentration can affect the rate of reaction. My experiment will be conducted to find out at what concentration does sodium thiosulphate with hydrochloric acid have the most reaction and how the concentration generally affects the rate of reaction. Particle size has a big impact on the speed of a reaction, if the particles are big then the reaction would be slow but if the particles are small the reaction will be fast. A catalyst often changes a reaction rate and they increase the speed of reaction always. The rate of reaction for this experiment will be measured by timing how long it takes for the sulphur from the sodium thiosulphate to cover an 'x' under a beaker. To test the rate of reaction and what affects it, we could have tested the effect of ph on rate of reaction, but that was not complicated enough. We used: * Sodium thiosulphate * Water * Hydrochloric acid Dilute sodium thiosulphate with water according to these measurements: Concentration HCL THIO H2O 00% 20ml 60ml 0ml 75% 20ml 45ml 5ml 50% 20ml 30ml 30ml 40% 20ml 24ml 36ml 25% 20ml 45ml 5ml How we carried out the investigation ) Prepare equipment 2)

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Temp labreport

How Temperature of HCL Effect Rate Of Hydrogen Produced Aim:- To determine how temperature affects the rate at which the reaction between Magnesium ribbon (Mg) and Hydrochloric acid (HCl) takes place. Introduction:- The rate of reaction can be affected by a number of factors: temperature, concentration, adding a catalyst and surface area. The one that I am going to be investigating and explaining about is temperature. Changes in temperature change the kinetic energy of the particles and hence the numbers of successful collisions with enough energy to break existing bonds and make products. For a reaction to take place, molecules must collide with each other. When they do so, they must possess enough energy to break the intermolecular bonds and hence, cause a reaction. The two theories that affect temperature and the rate of reaction are the kinetic theory and the collision theory. The kinetic theory clearly states that the positioning and movement of particles in a substance increases if the temperature increases. Therefore, increasing the temperature increases the energy between the particles and makes them move around a lot more and collide more often. Hypothesis: - The rate of reaction has a positive relationship with the temperature of the Hydrochloric Acid. Apparatus:- ) Test tube 2) Rubber tube (a.k.a. delivery tube) 3) Measuring cylinder X2 [1-10ml, 1-100

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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

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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

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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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