I then measured to see how long it would take to gain 100 cm3 of CO2 using a stopwatch and a gas syringe. To make sure the gas syringe is working properly I must make sure that the clam is not on too tight or it will affect the outcome of the results. To obtain the most reliable results I will do each experiment three times. [IMAGE]I predict that the high molarity concentration solution will have a much faster rate of reaction than the weaker solution. I have predicted this from my knowledge of a previous experiment and scientific knowledge.
Rates Of Reaction Investigation Plan: This experiment is planned to investigate the rate of reaction when mixing Copper sulphate (CuSO4) with Zinc powder (Zn). My plan is to see what happens before, during and after the reaction takes place. I will need the following equipment to carry out this investigation: Ø A 50ml marked measuring tube Ø A digital precision scale Ø 600ml of copper sulphate Ø A digital thermometer Ø A pot of Zinc powder Ø A sandpaper (to sand the Copper sulphate off the thermometer) Ø A pen and a paper (to record results.) Ø A beaker (to mix the elements) Ø A stirring stick For the first preliminary results chart, the variable will be the amount of Zinc powder but the copper sulphate solution will be 30 ml. Step-by-step: In order to get satisfactory results out of this experiment, you'll have to follow carefully the step-by-step instructions: i.
There are several methods that can be used to find the order of reaction: · I could use an excess of magnesium ribbon and note down how much gas has evolved every 10 seconds until the reaction has finished. · I could repeat the same procedure as above, but with an excess of acid instead of magnesium ribbon. · I could use an excess of acid and change the concentration, this would not require the reaction to be completed so I would have to time how long it takes for a set amount of hydrogen gas to form. There are several chemical equations that are relevant to this investigation:- Mg(s) + 2HCl(aq) MgCl2(aq) + H2(g) Mg(s) + H2SO4(aq) MgSO4 + H2(g) Mg(s) + 2CH3CO2H(aq) Mg(CH3CO2)2(aq) + H2(g) 3Mg(s) + 2H3PO4(aq) Mg3(PO4)2(aq) + 3H2(g) In my experiments I will not be using phosphoric acid due to time restrictions and it is not relevant to the problems I am discussing, because it is a tribasic acid and I am comparing monobasic and dibasic acids. The equation needed to find the activation energy in a reaction is called the Arrhenius equation.
Zinc and Hydrochloric-Acid Abstract: We observed the reaction between zinc and hydrochloric acid and recorded it in a table and learned wether the percentage of zinc is effected by the amounts of both substances added to the solution. Introduction The purpose of this experiment is to determine if the amount of zinc and hydrochloric acid will effect the percentage of the zinc in the out coming solution. We are reacting zinc metal with hydrochloric acid to produce a compound of zinc and chlorine atoms. We are then recording our data and observations and place it in a logical data table. Purpose The whole purpose of this experiment is to determine wether or not the amount of the zinc and or hydrochloric acid effects the out coming percent of the solution after under going chemical reaction.
PURPOSE To investigate the reactions of a typical acid (dilute hydrochloric acid) with metals, metal oxides, carbonates and bases. APPARATUS The following materials in order to complete this experiment: Dropper bottles containing 0.1M solutions of hydrochloric acid or limewater (calcium hydroxide) and sodium hydroxide. Dropper bottle of bromothymol blue indicator Small samples of the following metals: zinc, copper turnings, magnesium and iron Copper (II) oxide powder Magnesium oxide Marble chips (calcium carbonate) Sodium carbonate 12 test tubes and test tube holder Bunsen burner Stopper or cork Wax taper and matches PROCEDURE (a) REACTION WITH METALS Place a small piece of magnesium ribbon in a test tube and add about 2mL of dilute HCL. Stopper the test tube and allow the gas to accumulate. Remove stopper and test for the gas that evolved by holding a lighted taper to the mouth of the test tube.
Nitrogen oxide spoils the environment when it reacts with oxygen; however, the catalytic converter breaks it up, reducing the amount of nitrogen oxide being released. In the reaction 2CO + O2 → 2CO2, oxygen is added to carbon monoxide to create carbon dioxide, which is practically harmless. Oxygen is also added in the reaction CxH2x+2 + [(3x+1)/2]O2 → xCO2 + (x+1)H2O to unburnt hydrocarbons in order to create carbon dioxide and water, which are again harmless. Catalytic converters play a major role in assisting in the reactions in order to change the products by rearranging and breaking up the
Our procedure though was not without its mistakes. These mistakes are vital because they affect the data we conclude. Theoretically, according to the balanced chemical equation, for every mole of hydrated cobaltous chloride that is being heated, the decomposition ensures that the compound decomposes into one mole of cobalt(II) chloride and six moles of gaseous water vapor. Thus, in theory we should lose the mass equal to six moles of water vapor in each trial. Unfortunately, this is not the case because we don’t have perfect lab conditions and factors such as the time heated, utilization of the same crucible, and the inconsistency of magnitude of the flame from the Bunsen burner all contribute to differences in mass percent change for each
One of the strips was put into each tube and then timed with a stop clock and the level of froth was measured as it rose up the side of the tube every 20 seconds until the froth started to fall. This was done to each tube individually so that a more accurate measurement was taken. Results See Overleaf. Conclusion The enzymes were at low activity at around 0oC and then a slight rise all the way up to 40oC (gentle curve), followed by a steep downward curve or slow in activity up ... ... middle of paper ... ...at the surface area would not be equal all the way through the experiment. A small surface area error would probably lead to a large rate of reaction mis-calculation.
----------- I predict that the higher the concentration of sodium thiosulphate, the quicker it will react... ... middle of paper ... ...the result of this mix up, as maybe some residue remained in the burette, even after rinsing. If there had been sufficient time, this result would have most certainly have been taken again. The small red marks protruding from the points on my graph are attempted error bars. However, with the exception of the anomalous result, these were so absurdly small they are all but indiscernible. Stability of conclusion.
Several metal carbonates were placed in a test tube and linked to a syringe that measured the amount of carbon dioxide gas when the metal carbonates were heated. This experiment is to see how fast metal carbonates will break down to produce carbon dioxide. The reason they break don’t break down at the same time is because more reactive ones don’t want to break up. So the longer it holds onto its carbonate the more reactive the metal is. In this experiment there are a few factors that can affect the results of the experiment.