How does surface area affect reaction speed? The aim of this experiment was to investigate how the surface area affects the rate of a reaction in between calcium carbonate and hydrochloric acid. My hypothesis was that if the surface area to volume ratio of calcium carbonate was increased, then the rate of the reaction will increase because there are more particles that are accessible by the hydrochloric acid, thus more particles that can react with each other. Variables Independent- Surface area of calcium carbonate Dependent- Amount of carbon dioxide produced (cm3) Controls- Amount of calcium carbonate (g) Volume of hydrochloric acid (ml) Same beaker Same concentration of HCl Same temperature of both HCl and …show more content…
The reason why the chips were so slow was because it had a very small surface area to volume ratio. Each granule had a high surface area to volume ratio and each powder had a very high ratio. The reason why the difference between the granules and the powder was not a lot was because each granule was pretty flat, and quite a lot of calcium carbonate molecules were accessible by the hydrochloric acid. If the granules had been less flat, the difference would be higher. The graph of the powder shows how a lot of gas produced in the beginning and then exponentially decayed. This is because less calcium carbonate atoms were present and they the small clumps might have clumped together. Our original method was to use a gas syringe; however a small bit of liquid somehow got into the syringe, making the plunger very hard to move. After waiting 10 minutes, we realized the gas wasn’t able to push the plunger and so we had to change our method quickly. The other method was much more reliable, as in it wouldn’t stop working. One down side to it was that the powder/granules should have been stirred constantly, to ensure them calcium carbonate not clumping together. Also, none of the reactions completed, so we can’t see how much gas is produced during an entire reaction. It is impossible to say whether or not this experiment was reliable because we only did it once. However, this experiment is
If the concentration of the solution is increased the particles have less room to move around which creates a greater chance of collisions. The surface area of the reactant greatly affects the speed of which it reacts because if the reactant is grinded up or cut up the solution has more room to get to it. The reaction rate can be calculated by the formulae; rate of reaction = total amount of reactant used or product made ÷ time taken. (Collision theory and rates of reaction, 2013)
Rate of reaction between Hydrochloric Acid and Calcium Carbonate Calcium carbonate reacts with hydrochloric acid to form carbon dioxide gas. One way of following the rate of reaction at which it reacts is to measure the volume of carbon dioxide produced at certain time intervals during the reaction. CaCO + 2HCl CaCl + H O + CO = = =
Three factors that can affect the rate of reaction are temperature, pH and the salinity.
* By using the dropper and measuring cylinder, 7 ml sodium carbonate solution was added to the test tube
Introduction: The rate expression for this reaction is of the form: rate = K(CV+)M(OH-)N Where k = re constant, m is the order of the reaction with respect to the concentration of CV+, and n is the order of the reaction with respect of OH-. In the experiment the concentration of OH- is purposely made 1000 times larger then Concentration of CV+. Thus, the concentration of OH- changes so little during the
As the substrate in increased the initial reaction rate will increase until it is fully submerged and then will not increase any more. The relationship is linear. As the substrate concentration increases, the initial reaction rate increases.
Discussion The purpose of this lab was to measure the mass of a solid reactant, in this case, NaHCO3, which is also known as baking soda, and to find the mass of the solid product NaCl (salt) as well. From there, the masses were to be converted into moles and created into ratios that showed the relationship between the reactants and products. That information was then compared to the theoretical data in order to check its accuracy and reveal the significance of mole ratios in chemical reactions.. During the experiment, hydrochloric acid (HCl) was added to the baking soda in order to begin the reaction.
The term concentration refers to the amount of a substance present in a certain volume of liquid or gas. Increasing the concentration of the reactants will increase the rate of the reaction. If the concentration of a reactant in a solution is increased, there will be a greater number of particles in a given volume of solution. This means the particles are more likely to collide and therefore react when there are more of them. Collisions between particles are necessary for the reactants to rearrange and form the products. In this experiment, the rate of the reaction between magnesium ribbon and hydrochloric acid will be increased by adding a higher concentration of hydrochloric acid each time. The chemical equation between magnesium ribbon and hydrochloric acid can be written as:
From the results that were acquired from mixing the liquid reagents with each powder, it was determined that Unknown Mixture #1 consisted of baking soda and cornstarch. When individually testing the substances from Unknown Mixture #1 with the liquid reagents, a few noticeable reactions occurred. Mixing baking soda with vinegar caused bubbling to occur. This is because a neutralization reaction took place between the two reactants. In this reaction, sodium bicarbonate(baking soda) reacts with vinegar and produces sodium acetate, water, and carbon dioxide(HC2H3O2(aq) + NaHCO3(aq) NaC2H3O2(aq) + H2O(l) + CO2(g) ). The gaseous carbon dioxide most likely tried to escape into the atmosphere and caused the bubbling to occur. Another noticeable reaction
In this experiment we tested the effects that enzymes and substrate have on chemical reaction rates, which is the rate at which chemical reactions occur.. This experiment tested how different concentrations of enzyme and substrate affected the light absorption measurements on a spectrophotometer. The experiment also tested how temperature affected the light absorption, and in a separate test, the effect of the enzyme inhibitor hydroxylamine was also tested. In the first test conducted, 3 different concentrations of enzyme, and three different concentrations of substrate were measured in a spectrophotometer. For the enzyme and the substrate, the measurements got higher as the concentrations were higher, but the over measurements of the substrate were smaller than those of the enzyme. In the second test conducted, the medium concentration enzyme was tested under the temperatures; 4°C, 23°C, 37°C, and 60°C. The measurements in this test got higher as the temperature got higher, but did the measurements under 4°C were overall significantly higher than the other temperature measurements. Lastly, the last test conducted showed that the measurements of the substance with 0 and 1 drop of hydroxylamine inhibitor went up, but the measurements of the enzyme with 5 drops of hydroxylamine inhibitor stayed rather low and did not change much. In conclusion, these experiments showed that chemical reaction rates are sped up with higher concentrations of enzyme, substrate,
1. In the lab activity the rate of the reaction would slow down because it is harder to find unbroken toothpicks since the amount is decreasing because there are less substrates present. 2. By starting off with 400 times more than 50 toothpicks (increased) from the start, than the reaction rate can keep on getting faster and faster because the enzyme would have more to react in the process.
3. Please refer to the graphs at the beginning of the post-lab and question 2a. The effect of magnesium on a reaction rate depends on the magnesium’s shape and surface area, greater the surface area, the faster the reaction rate.
An unknown sample was massed and put into three test tubes for three different trials. A gas transfer assembly was put together and hydrochloric acid was added to each sample in each test tube. A reaction between the carbonate sample and the acid occurred and the volume of carbon dioxide gas produced was recorded. This process was repeated three times. The mass
The rate of a reaction varies at different temperatures and reactant concentrations. In this experiment, the orders and dependence of the rate constant of the products used are determined by the following chemical reaction:
5. From your data in Table 3, explain the difference in time between the three solutions.