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.

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 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?

In a reaction energy diagram, which point or segment represents the enthalpy change (ΔH) of the reaction?

Which of the following represents the standard heat of formation reaction for sodium chloride (NaCl) in its solid form?