Given is the following information for the reaction of magnesium oxide and magnesium with hydrochloric acid in a coffee cup calorimeter. (Atomic masses : Mg = 24.3, O = 16.0 g/mol, respectively) i Weight of Magnesium Oxide used 0.750 g ii mols of Magnesium Oxide used ? iii ∆Tcalorimeter 3.5°C iv qcalorimeter = Ccal x ∆T [Ccal = 418J(g●°C] ? v qreaction ?
Given is the following information for the reaction of magnesium oxide
and magnesium with hydrochloric acid in a coffee cup calorimeter.
(
|
i |
Weight of Magnesium Oxide used |
0.750 g |
|
ii |
mols of Magnesium Oxide used |
? |
|
iii |
∆Tcalorimeter |
3.5°C |
|
iv |
qcalorimeter = Ccal x ∆T [Ccal = 418J(g●°C] |
? |
|
v |
qreaction |
? |
|
i |
Weight of Magnesium metal used |
0.725 g |
|
ii |
mols of Magnesium metal used |
? |
|
iii |
∆Tcalorimeter |
22.0°C |
|
iv |
qcalorimeter = Ccal x ∆T [Ccal = 418J(g●°C] |
? |
|
v |
qreaction |
? |
|
H2(g) + ½O2(g) → H2O(l) |
-285.8 kJ |
Now, calculate the ∆H for the following reactions in kJ /mol.
MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(l)
Mg (s) + 2HCl(aq) → MgCl2(aq) + H2 (g)
Using all the above information and data, calculate the ∆H for the following
reaction:
Mg (s) + ½O2(g) → MgO(s) ∆H = ?
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