Using the provided table and the equation below, determine the heat of formation (in kJ/mol) for PbS. 2 PbS (s) + 3 O2 (g) → 2 SO₂ (g) + 2 PbO (s) AH° = -828.4 kJ/mol Substance O₂ (g) SO: (g) PbO (s) Hf (kJ/mol) 0 -296.9 -217.3

The lattice energy is defined as the energy required to break one mole of an ionic solid into its ions in the gas phase. The lattice energy for calcium oxide corresponds to the following reaction. CaO(s) Ca2+(g) + O2-(g) DH = ? Using the following information, determine the lattice energy for calcium oxide. Ca(s) ----> Ca(g) DH = 178.2 kJ Ca(g) ----> Ca2+(g) + 2e-   DH = 1747.9 kJ O2(g) ----> 2O(g) DH = 498.3 kJ O2-(g) ----> O(g) + 2e- DH = -702 kJ Ca(s) + 1⁄2 O2(g) ----> CaO(s)   DH = -635.0 kJ   Using the unrounded answer from the previous problem determine q (kJ) for the following reaction when 1.00 grams of solid calcium oxide forms.     Ca2+(g) + O2-(g) ⟶⟶ CaO(s)

A chemist measures the enthalpy change AH during the following reaction: Fe(s) + 2 HCl(g) →FeCl₂(s) + H₂(g) Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction AH=157. kJ FeCl₂ (s) + H₂(g) → Fe(s) + 2HC1 (g) 2Fe (s) + 4H C1 (g) 3 FeCl₂ (s) + 3H₂(g) 2FeCl₂ (s) + 2H₂(g) 3Fe (s) + 6HCl (g) ΔΗ [ kJ kJ kJ 0x x10 × Ś

Using standard heats of formation, calculate the standard enthalpy change for the following reaction. 2HBr(g) + Cl₂(g) → 2HCl(g) + Br₂(g) AH (HBr(g)) = -36.3 kJ/mol AH (Cl₂ (9)) = 0.0 kJ/mol AH (HCl(g)) = -92.3 kJ/mol AH (Br₂ (9)) = 30.9 kJ/mol AH rxn = kJ

A scientist measures the standard enthalpy change for the following reaction to be -737.2 kJ : 2Co(g) + 2 NO(g)2CO2(g) + N2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CO(g) is kJ/mol.

Consider the balanced reaction 4 A + 9 B → 8 C + 8 D and the enthalpies of formation provided in the table below. AH Compound (kJ/mol) A 170.8 231.1 D -98.4 Suppose that the AH of the overall reaction is -2,029.3 kJ/molxn. Calculate the value of the AHf of C in kJ/mol. Report your answer to three decimal places (ignore significant figures).

（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g)     ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A?   （2）Consider the reaction: C (s) + O2 (g) → CO2 (g)     ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?

Consider the following balanced reaction: 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g)          ΔHrxn = -1124.0 kJ Calculate the enthalpy of formation (in kJ/mol) for H2S(g). Given: The standard enthalpies of formations (ΔHof) of H2O(l) and SO2(g) are -285.8 kJ/mol and -296.8 kJ/mol, respectively. IMPORTANT: Enter both the sign and the value (no units), using 1 decimal place (e.g. -999.9) Consider the following balanced reaction: 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g)          ΔHrxn = -1124.0 kJ Calculate the enthalpy of formation (in kJ/mol) for H2S(g). Given: The standard enthalpies of formations (ΔHof) of H2O(l) and SO2(g) are -285.8 kJ/mol and -296.8 kJ/mol, respectively. IMPORTANT: Enter both the sign and the value (no units), using 1 decimal place (e.g. -999.9)