AS is negative for the reaction O CH3OH (1)→ CH3OH (g) O C6H12O6 (s)→ 6C (s) + 6H2 (g) + 302 (9) O 2H₂O (g) → 2H2 (g) + O2 (9) O Sr(NO3)2 (aq) + 2LiOH (aq) → Sr(OH)2 (s) + 2LiNO3 (aq) - OLIOH (aq) → Li+ (aq) + OH(aq) -

Given these reactions, where X represents a generic metal or metalloid 1) H, (g) + 0,(g) H,O(g) ΔΗ = -241.8 kJ 2) X(s) + 2 Cl, (g) → XCl,(s) ΔΗ = +288.1 kJ 3) H,(g) + ¿Cl,(g) → HCI(g) ΔΗ -92.3 kJ 4) X(s) + O,(g) → XO,(s) AH4 = -529.5 kJ 5) Н, О(g) — н,О() H,O(1) AH5 = -44.0 kJ what is the enthalpy, AH, for this reaction? XCI, (8) + 2 H,О0() — ХО,(s)+4 HC(g) 141.62 ΔΗ kJ %3D Incorrect

Calculate the standard enthalpy change for the reaction 2Al(s) + Fe2O3(s) → 2Fe(s) + Al2O3(s) given that 2Al(s) + 3O2(g) → Al2O3(s) ΔH = –1669.8 kJ/mol 2Fe(s) + 3O2(g) → Fe2O3(s) ΔH = –822.2 kJ/mol ΔH = ?

The standard enthalpy change for the following reaction is -56.0 kJ at 298 K. Na(s) + 1/2 H₂(g) → NaH(s) ΔΗ° = -56.0 kJ What is the standard enthalpy change for the reaction at 298 K? 2 NaH(s) → 2 Na(s) + H₂(g) kJ

Determine the enthalpy (in kJ/mol) for the reaction 3 SiCl₄ (s) + 4 Fe (s) → 4 FeCl₃ (s) + 3 Si (s) (Please show steps)

The bombardier beetle uses an explosive discharge as a defensive measure. The chemical reaction involved is the oxidation of hydroquinone by hydrogen peroxide to produce quinone and water:

Do the follow reactions depict Heat of Formation Reactions? If so, mark the reaction as YES, if it is not a Heat of Formation Reaction, then choose NO. ✓3/2 H₂(g) + P(s) → PH3(g) H₂(g) + 1/2O₂(g) → H₂O(g) Al(s) + 3/2 Br₂(1)→ AlBr3(S) Na(s) + H₂O(1)→ NaOH(aq) + 1/2 H₂(g) ✓2As(s) + 5/2 O₂(g) → As2O5(s) In formation reactions the reactants must be elements in their most common states, and the only product is one mole of the substance of interest.

Calculate the standard enthalpy for the reaction: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g), given the following data: N2(g) + O2(g) → 2NO(g) ΔHrxn = -43.1 kcal mol-1   N2(g) + 3H2(g) → 2NH3(g) ΔHrxn = -21.9 kcal mol-1   2H2(g) + O2(g) → 2H2O(g) ΔHrxn = -115.6 kcal mol-1   Round your answer to 2 decimal places.

In a coffee-cup calorimeter, 110.0 mL of 1.2 M NaOH and 110.0 mL of 1.2 M HCl are mixed. Both solutions were originally at 22.5°C. After the reaction, the final temperature is 30.5°C. Assuming that all the solutions have a density of 1.0 g/cm³ and a specific heat capacity of 4.18 J/°C.g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. AH = 0.182 kJ/mol

Determine the energy associated with each of these processes in order to recycle 1.26 mol Cu. The smelting of copper occurs by the balanced chemical equation: CuO(s)+CO(g)Cu(s)+CO2​(g)where ΔH°f,CuO is = –155 kJ/mol. Assume the process of recycling copper is simplified to just the melting of the solid Cu starting at 25°C. The melting point of Cu is 1084.5°C with ΔH°fus = 13.0 kJ/mol and a molar heat capacity, cP,Cu = 24.5 J/mol·°C.