How do I calculate the enthalpy change per mol of magnesium?
Equation given:
Mg(s) + 1/2 O2 (g) ---> MgO(s)
Magnesium reacts in acid to form hydrogen gas and a salt:
Mg(s) + 2HCl (aq) ---> H2 (g) + MgCl2 (aq) ∆H1 =? KJ
Magnesium oxide reacts in acid to form water and a salt:
MgO(s) + 2HCL (aq) ----> H2O (l) + MgCl2(aq) ∆H2 =? KJ
Hydrogen and oxygen gases react to form water:
H2 (g) + 1/2O2 (g) ----> H2O(l) ∆H2 = -285.8 KJ
From the experiment I got:
Mass Of magnesium 0.04g
Hydrochloric Acid 100.0mL
Initial Temperature 20˚C
Final Temperature 24.1˚C
Mass of magnesium oxide 0.99g
Hydrochloric acid 100.0mL
Initial Temperature 20˚C
Final Temperature 30˚C
Equation given:
Mg(s) + 1/2 O2 (g) ---> MgO(s)
Magnesium reacts in acid to form hydrogen gas and a salt:
Mg(s) + 2HCl (aq) ---> H2 (g) + MgCl2 (aq) ∆H1 =? KJ
Magnesium oxide reacts in acid to form water and a salt:
MgO(s) + 2HCL (aq) ----> H2O (l) + MgCl2(aq) ∆H2 =? KJ
Hydrogen and oxygen gases react to form water:
H2 (g) + 1/2O2 (g) ----> H2O(l) ∆H2 = -285.8 KJ
From the experiment I got:
Mass Of magnesium 0.04g
Hydrochloric Acid 100.0mL
Initial Temperature 20˚C
Final Temperature 24.1˚C
Mass of magnesium oxide 0.99g
Hydrochloric acid 100.0mL
Initial Temperature 20˚C
Final Temperature 30˚C