Investigation on the rate of reaction of metals with acids i am using hydrochloric and ethanoic with magnesium

Question

i need help i figured out hydrochloric with mgnesuim gives 2nd order but stuck on what ethanoics order of reaction is could help me with this experiment.i am using 15cm3 of acids and 0.17g of magnesuim ribbon in an gas stringe experiment.

Answer 1

Rate = k [A]^x[B]^y
is the general rate equation.
The equation between Mg and ethanoic acid is

Mg(s) + 2CH3COOH = Mg(CH3COO)2 + H2(g)

Again using the gas syringe collect the H2 and note the volumes at different times. This will give the 'rate'. You also need to know the initial concentration of ethanoic acid in order to calculate the rate constant 'k'. As a general rule if two moles of a substance are required then the concentration in the rate equation is raised to the power '2'
Similarly to HCl you require '2' moles of CH3COOH to one mole Mg.
As the reaction proceeds the concentration of CH3COOH becomes less. The Mg ribbon does not affect the rate.
Rate = k [Mg]^0[CH3COOH]^2
NB [Mg]^0 = 1 (anything to power zero = 1).

Rate = k[CH3COOH]^2

Hope this helps!!!!