Investigating Effects Of Molarity Of Hydrochloric Acid

On Calcium Carbonate Essay, Research Paper

AimIn this investigation I am aiming to find out how the

concentration of acid affects the rate of reaction with Calcium Carbonate

(Limestone).HypothesisI predict that the higher the concentration of acid then

the faster the rate of reaction.Calcium

Carbonate + Hydrochloric Acid => Carbon Dioxide + Calcium Chloride ????????????????

CaCO3??????? +???????? 2HCl?????????????????? =>??????????

CO2???????????? +????? H2O? +? CaCl2???? I

predict this because when a chemical reaction takes place, the atoms are broken

loose from their arrangements and re-arranged into different groupings, forming

new substances. The reaction above can only happen if the particles of acid

came into contact with particles of limestone. In gases and liquids or in

solutions, the particles are moving around freely and can bump into each other

more easily. ???? In this reaction of acid and limestone, if

the acid is very concentrated this means that there will be plenty of acid

particles close together in the solution. Acid particles bump into the calcium

carbonate very frequently and if they do this, the surface of the limestone

will dissolve quickly. If the acid is very dilute then the particles will be

more spread out. They will bump into the limestone a lot less often and so the

reaction will take longer. A general rule could be:If

the solution is more concentrated, the reaction will be fasterIn this

reaction, the limestone is a solid. Therefore the particles in a solid cannot

move around freely and only the particles on the surface of the limestone can

react with the acid. The diagrams on the next page show the same mass of

limestone. On the left hand side diagram, there is one lump of limestone. On

the right there are several smaller pieces: VariablesThe variables I

will be considering are:?Pressure at which the experiment ensues. ?Surface area of the limestone chip(s). ?Temperature

at which the reaction takes place. ?Volume

of acid. ?Molarity

of acid. ???? Each of the

variables above affects the rate of reaction in their own ways. The pressure of

the experiment causes the reaction to occur quicker as with more pressure there

will be more gaseous particles and less space for the particles, so the

particles will strike each other more frequently. With the Surface area of the

limestone chip(s), there will be more for the acid particles to react with, as

the total surface area will be more thus more particles of the limestone chip.

The temperature at which the reaction happens does not really have an effect in

this case, but it can be an important variable in another investigation. ???? The volume of acid will make a difference

but only up to a certain point as if you keep adding acid then the particles

will just keep increasing but if too many acid particles are added then the

acid particles bump into each other as well as the limestone. Molarity of acid

is a key aspect in this experiment as if I use an acid with higher molarity

there will be more acid particles to react with the limestone surface and so

there will be more chance of collision. MethodI set up my

apparatus as on the next page. Once everything had been set up I got 2.00 grams

of limestone chip(s) and I put them into a conical flask. I decided on 2.00

grams of limestone through a preliminary process which consisted of testing and

making our own judgements to see if we could get a reasonable volume of carbon

dioxide, if I was to use too much limestone or too much acid then the reaction

will produce too much gas too quickly. If there was not enough limestone or

acid then not enough gas will be produced. That is why I used 2.00 grams of

limestone and 15ml of acid, as they seemed to work well with each other. Once I

added the 15ml of Hydrochloric acid to the limestone in the conical flask I put

a bung on top of it and started the stopwatch. I measured the volume of gas

collected in a measuring cylinder and timed the experiment for 2 minutes. I

collected the gas in a measuring cylinder but this is not an entirely accurate

technique of recording results, but they were the only instruments available to

me. ???? I repeated this process again for 0.5 molar

acid, 0.75 and 1 molar acid. I kept the volume of acid and the mass of

limestone the same for each experiment as to keep it a fair test. ???? Then I repeated the entire process again 3

times so that I could get average results. During my experiment I managed to

control all the variables to the best of my ability. I recorded all my results

in a table, which you can also see later on in the coursework, and using the

results I will also draw a graph. Results Volume of gas collected after 2 minutes Attempts Concentration of Acid 1 2 3 Average 0 0 0 0 0 0.25 6 5 6 5.6 0.5 9 11 14 11.33 0.75 16 16 13 15 1 23 20 18 20.3 Analysis Below is the working out fo

Внимание, отключите Adblock

Вы посетили наш сайт со включенным блокировщиком рекламы!
Ссылка для скачивания станет доступной сразу после отключения Adblock!

Скачать