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What are the sources of errors in the experiment of determine of enthalpy change of hydration of copper ii sulphate six?
Wiki User
∙ 11y ago
heat loss to the surroundings if you using the simple 'insulated cup' method. Insufficient stirring, so that not all the solid is dissolved is another. A 'chemical' source of error is that the anyhydrous salt, which forms one half of the experiment, may not be completely anhydrous and will also absorb water from the air if left exposed for any length of time.
Wiki User
∙ 11y ago
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What is color of ferric sulphate?
The colour depends on the degree of hydration, but it is most often green.
Why do you need to use a freshly prepared ironII sulphate in our lab experiment?
Ferrous or iron(II) compounds can easily be oxidised to ferric or iron(III) compounds, when exposed to air. So iron(II) sulphate which is stored for some time will have iron(III) sulphate present.
What elements make up copper sulfate?
The elements in copper sulphate are copper, sulphur and oxygen. Copper sulphate is a compound, made up of three elements. The symbol for this compound is CuS04.
Balance Copper 2 sulfate pentahydrate is heated to drive off the water hydration?
penta = 5 copper(II) sulphate pentahydrate = CuSO4*5 H2O CuSO4*5 H2O + heat --> CuSO4 + 5 H2O
What is the common name for hydrogen sulphate?
hydroxic sulphate
What is the standard enthalpy for sodium sulfate?
The standard enthalpy for sodium sulphate is -1387kJ/mol.
What is color of ferric sulphate?
The colour depends on the degree of hydration, but it is most often green.
What is the purpose of using anhydrous magnesum sulphate in the experiment?
removing water
Why is enthalpy of solution of 4g of anhydrous copper sulphate lower than the expected value?
Firstly, what do you mean by "lower"? Do you mean less exothermic? If that is what you mean, then one possible reason is that your anhydrous copper sulphate was not truly anhydrous, and that is highly likely. Did it look a bit blue? If so then it had absorbed some water from the air and therefore you did not weigh out as many moles of it as you had thought - hence less heat was released in your experiment.
What has the author George Walton written?
George Walton has written: '1. The nature of the variable hydration of precipitated barium sulfate. 2. The contamination of precipitated barium sulfate by univalent cations ..' -- subject(s): Barium sulphate, Precipitation (Chemistry), Cations, Hydration
How do you determine the colorimetric estimation of unknown copper sulphate concentration in solution?
by colourimetry
What will happen if you put copper sulfate on a turtle?
Probably a very dilute solution of copper sulphate act as a desinfecting agent; but the copper sulphate is toxic. It is more sure to avoid this experiment.
Why do you need to use a freshly prepared ironII sulphate in our lab experiment?
Ferrous or iron(II) compounds can easily be oxidised to ferric or iron(III) compounds, when exposed to air. So iron(II) sulphate which is stored for some time will have iron(III) sulphate present.
What chemical bond possess low latent heat of fusion?
Latent heat of fusion (or enthalpy of fusion) is a characteristic of a substance, rather than a chemical bond. If you mean enthalpy of reaction then the lowest absolute values are for the bonds in H2, F2, and Cl2 as gases, which are zero. One low (and negative) value is for cuprous sulphate. Please see the link.
Chemistry of SRC cement?
Sulphate resisting cement:Low C3A ContentLow C4AF contentCa(OH)2 + SO2 ---> CaSO3 + H2OIn the above equation water is evolved, so hydration process is continuous in SRC
What elements make up copper sulfate?
The elements in copper sulphate are copper, sulphur and oxygen. Copper sulphate is a compound, made up of three elements. The symbol for this compound is CuS04.
Why enthalpy change of hydration of magnesium sulphate cannot be measured directly?
Because this kind of reaction is usually not spontaneous. Heating maybe required to provide the required activation energy. Heating on the other hand would introduce heat change and thus a higher temperature change to the system. As a result the actual temperature change caused by the reaction is hard to measure.
