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?

When 1.550 g of liquid hexane (C6H14) undergoes combustion in a bomb calorimeter, the temperature rises from 25.87 °C to 38.13 °C. If the heat capacity of the bomb calorimeter is 5.73 kJ/°C, what is the ΔErxn for the reaction in kJ/mol hexane?

When 3.50 g of Ba(s) is added to 100.00 g of water in a container open to the atmosphere, the reaction shown below occurs and the temperature of the resulting solution rises from 22.00°C to 47.40°C. If the specific heat of the solution is 4.18 J/(g °C), calculate the heat absorbed by the solution.

When 8.00 g of Ba (s) is added to 100.00 g of water in a container open to the atmosphere, the reaction shown occurs and the temperature of the resulting solution rises from 22.0°C to 77.62°C. If the specific heat of the solution is 4.18 J/(g°C), calculate ΔH for the reaction. Assume no heat is lost to the surroundings.

When iron metal is mixed with hydrochloric acid, the following reaction occurs: 2Fe(s) + 6HCl(aq) → 2FeCl3(aq) + 3H2(g). When 1.104 g of iron is mixed with 26.023 g of HCl in a coffee cup calorimeter, the temperature rises from 25.2°C to a final temperature of 32.5°C. What is the enthalpy change (ΔH) for the reaction per mole of iron, assuming the specific heat capacity of the solution is 4.18 J/g°C and the total mass of the solution is 100.0 g?

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.