8. Thermochemistry

Which of the following is the correctly balanced thermochemical equation for the combustion of methane (CH₄) with oxygen (O₂) to form carbon dioxide (CO₂) and water (H₂O), given that the enthalpy change is -890 kJ/mol?

Calculate the enthalpy change, ΔHrxn, for the neutralization of HCl with NaOH, in kJ per mole of HCl neutralized, given that the temperature change is from 20°C to 27°C and 37.50 mL of 1 M NaOH and 37.50 mL of 1 M HCl were used.

Calculate the heat of combustion of ethane (C2H6) using the following thermochemical equation: C2H6 + 3.5 O2 -> 2CO2 + 3H2O. Given the standard heats of formation for ethane gas, carbon dioxide gas, and water liquid are -84.7 kJ/mol, -393.5 kJ/mol, and -285.8 kJ/mol, respectively.

If 24.0 grams of carbon monoxide (CO) undergoes complete oxidation to form carbon dioxide (CO2), how much heat is released, assuming the reaction is exothermic? The balanced equation is: 2CO(g) + O2(g) → 2CO2(g), ΔH = -566 kJ/mol.

What final temperature will 120 g of benzene at 7°C have after it absorbs 2.20 kJ of heat? The specific heat capacity (Cp) of benzene is 1.74 J/g°C.

What is the change in enthalpy in kilojoules when 3.20 mol of Mg is completely reacted according to this reaction: 2Mg(s) + O2(g) -> 2MgO(s)? ΔH = -1204 kJ

When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF, CaF2 precipitates, as shown in the net equation below. The initial temperature of the solution is 30.0 °C. Assuming that the reaction goes to completion, and that the resulting solution has a mass of 100.0 g, what is the enthalpy change (ΔH) for the reaction if the final temperature of the solution is 25.0 °C?