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HCL and MG
Aim
The aim of this investigation is to find out the effect of concentration of acid, in the
reaction between dilute hydrochloric caid and magnesium ribbon. ...
The collision theory describes how the rate of reaction increase (the time taken for the
magnesium ribbon to disappear when it is reacted with hydrochloric acid) when the
concentration of HCL increases. ...
Clearly, the time taken for the magnesium to disappear when it is placed in different
concentrations of HCL, is related in some way. The higher the concentration of HCL you
use, the less time it takes for the magnesium to disappear and so the rate reaction
increases. The concentraton of HCL you use is the independant variable because it will
vary, and the time taken for the rate of reaction to take place(i. ... The time it takes for the magnesium to disappear will be measured
accurately using a stop clock as soon as the HCL is poured into beaker with the
magnesium in it. ...
An equation for the reaction:
Magnesium + hydrochloric acid >magnesium chloride + hydrogen
Mg(s) + 2HCL(aq)>Mgcl2(aq) + H2(g)
1mole 2moles 1mole 1mole
So we can say that one mole of magnesium reacts with 2 moles of hydrochloric acid.
Approximate Word count = 2048
Approximate Pages = 8.2
(250 words per page double spaced)
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