These are the results that I have:
Between potassium carbonate and HCl
Mass of potassium carbonate used: 2.86 [g]
Initial temperature = 23degreesC
After mixing Potassium Carbonate with HCl = 25degressC
Change in T = 2C
Between potassium hydrogencarbonate and HCl
Mass of potassium hydrogencarbonate used: 3.30 [g]
Initial T = 2C
After mixing = 17.5C
Change in T = 2.5C
Now my questions are:
Calculate the enthalpy change for one mole of potassium hydrogencarbonate
(I found the enthalpy change between the KHCO3 and HCl by doing Q=mcdeltaT ->
Does this mean that I can just reuse my equation except solve for 1mole of KHCO3 or is the question not asking for the reaction between KHCO3 and HCl?)
What is the enthalpy change for the decomposition of potassium hydrogencarbonate?
(This one I have no clue on except I think I'm supposed to use Hess' law...)
Thanks to anyone who can help
Between potassium carbonate and HCl
Mass of potassium carbonate used: 2.86 [g]
Initial temperature = 23degreesC
After mixing Potassium Carbonate with HCl = 25degressC
Change in T = 2C
Between potassium hydrogencarbonate and HCl
Mass of potassium hydrogencarbonate used: 3.30 [g]
Initial T = 2C
After mixing = 17.5C
Change in T = 2.5C
Now my questions are:
Calculate the enthalpy change for one mole of potassium hydrogencarbonate
(I found the enthalpy change between the KHCO3 and HCl by doing Q=mcdeltaT ->
Does this mean that I can just reuse my equation except solve for 1mole of KHCO3 or is the question not asking for the reaction between KHCO3 and HCl?)
What is the enthalpy change for the decomposition of potassium hydrogencarbonate?
(This one I have no clue on except I think I'm supposed to use Hess' law...)
Thanks to anyone who can help
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