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c) Hess's law calculation of the enthalpy of formation of MgO Use Hess's law to calculate the enthalpy of formation of MgO, i.e., the reaction: Mg(s) + 1/2 O2(g) ? MgO(s) Use the two average enthalpy changes you measured in Part 2 for Equations (3) and (4) and the tabulated value of -285.8 kJ for the enthalpy of formation of liquid water (Equation (2)). Show work below. average enthalpy changes = 28.49 kJ/°C/mol 21.69 kJ/°C/mol equation 2: H2(g) + 1/2 O2(g) ? H2O(l) H = Hf, H2O = 285.7 kJ equation 3: Mg(s) + 2 HCl(aq) ? MgCl2(aq) + H2(g) equation 4: MgO(s) + 2 HCl(aq) ? MgCl2(aq) + H2O(l)

          c) Hess's law calculation of the enthalpy of formation of MgO
Use Hess's law to calculate the enthalpy of formation of MgO, i.e., the reaction:
Mg(s) + 1/2 O2(g) ? MgO(s)
Use the two average enthalpy changes you measured in Part 2 for Equations (3) and (4) and the tabulated value of -285.8 kJ for the enthalpy of formation of liquid water (Equation (2)). Show work below.
average enthalpy changes = 28.49 kJ/°C/mol
21.69 kJ/°C/mol
equation 2: H2(g) + 1/2 O2(g) ? H2O(l) H = Hf, H2O = 285.7 kJ
equation 3: Mg(s) + 2 HCl(aq) ? MgCl2(aq) + H2(g)
equation 4: MgO(s) + 2 HCl(aq) ? MgCl2(aq) + H2O(l)

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c) Hess's law calculation of the enthalpy of formation of MgO
Use Hess's law to calculate the enthalpy of formation of MgO, i.e., the reaction:
Mg(s) + 1/2 O2(g) ? MgO(s)
Use the two average enthalpy changes you measured in Part 2 for Equations (3) and (4) and the tabulated value of -285.8 kJ for the enthalpy of formation of liquid water (Equation (2)). Show work below.
average enthalpy changes = 28.49 kJ/°C/mol
21.69 kJ/°C/mol
equation 2: H2(g) + 1/2 O2(g) ? H2O(l) H = Hf, H2O = 285.7 kJ
equation 3: Mg(s) + 2 HCl(aq) ? MgCl2(aq) + H2(g)
equation 4: MgO(s) + 2 HCl(aq) ? MgCl2(aq) + H2O(l)

Added by Angelica O.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

05/31/2022

Step 1

Rearranged Equation 3: MgCl2(aq) + H2(g) -> Mg(s) + 2 HCl(aq) Rearranged Equation 4: MgCl2(aq) + H2O(l) -> MgO(s) + 2 HCl(aq) Now, we can add these two equations together: MgCl2(aq) + H2(g) + MgCl2(aq) + H2O(l) -> Mg(s) + 2 HCl(aq) + MgO(s) + 2 Show more…

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c) Hess's law calculation of the enthalpy of formation of MgO Use Hess's law to calculate the enthalpy of formation of MgO, i.e., the reaction: Mg(s) + 1/2 O2(g) → MgO(s) Use the two average enthalpy changes you measured in Part 2 for Equations (3) and (4) and the tabulated value of -285.8 kJ for the enthalpy of formation of liquid water (Equation (2)). Show work below. average enthalpy changes = 28.49 kJ/°C/mol 21.69 kJ/°C/mol equation 2: H2(g) + 1/2 O2(g) → H2O(l) H = Hf, H2O = 285.7 kJ equation 3: Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) equation 4: MgO(s) + 2 HCl(aq) → MgCl2(aq) + H2O(l)

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