apply hes's law to find the heat of Formation for MgO (s)
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Write the thermochemical equation for the standard enthalpy of formation of MgO(s). Use your data and Hess's Law to determine the value of ΔfH°(MgO).(Enter fractional coefficients as needed, e.g. 1/2 or 0.5 for 1/2) You will need the following piece of additional data: H2(g) + 1/2 O2(g) → H2O(l) ΔH° = -285.84 kJ Accepted literature value for MgO enthalpy of formation: -601.7 kJ Calculate the percent error in the MgO enthalpy of formation:
Supreeta N.
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)
Adi S.
Given the following data: Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) ΔH = -462 kJ MgO(s) + 2 HCl(aq) → MgCl2(aq) + H2O(l) ΔH = -146 kJ H2(g) + 1/2 O2(g) → H2O(l) ΔH = -286 kJ what is the heat of formation of MgO? Mg(s) + 1/2 O2(g) → MgO(s)
Suman K.
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