Abdul Rahman Khalifeh
Aim
To supervise the counterchange of the position of equilibrium between Co2+ (aq) of parsimony of 0.3 jetty L-1 and Cl- of closeness 3.0 mol L-1 when placed at temperatures of 0°C, 95°C and 25°C.
Hypothesis
Since this reaction is endothermic, as temperature increases the equilibrium will play to the right according to Le Chateliers principle. Water would move the equilibrium to the left and the HCl would move the equilibrium to the right according to Le Chateliers principle.
Variables
hooklike variable(s) | Independent Variable(s) | Controlled Variables |
The position of the equilibrium which is monitored by the colour change of the solution| The temperatures of 0°C, 25°C and 95°C. at which the reaction takes place| Same concentration of aqueous chloride ions (3.0 mol L-1)|
| | 6 test tubes of the same size, shape and volume.|
| | Same concentration of aqueous cobalt ions (0.
3 mol L-1)|
| | The same digital correspondence to 4 significant figures after the decimal point in order to have the same uncertainty for all measurements taken |
| | The same of solution in all cases|
Apparatus
starter| Chemicals| Equipment|
(3) evidence tube| 600 g of Ice| Goggles|
(3)50 cm3 Beaker| 30.0000 g of CoCl2.6H2O| Test tube holder|
Graduated cylinder- 100 cm3| Concentrated HCl | digital balance to 4 significant figures|
Conical Flask 100cm3| | bunsen burner burner|
| | Thermometer|
Method for the Control of Variables
In order to obtain the consummate control of variables we must control all other factors poignant the position of the equilibrium. Hence the concentration of aqueous chloride ions and aqueous cobalt ions must be fixed and this can be make by measuring the mass of CoCl2.6H2O accurately by utilize a digital balance to 4 significant figures. In order to control the...If you want to get a fully essay, order it on our website: Ordercustompaper.com
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