What will be the change in enthalpy when 100.0 g of butane, C4H10, is burned in oxygen according to the thermochemical equation: 2 C4H10(l) + 13 O2(g) → 8 CO2(g) + 10 H2O(g) with ΔH rxn = −5271 kJ?

Given the following thermochemical equation and data, calculate the standard enthalpy of formation (ΔH⁰f) for IF(g): IF7(g) + I2(g) → IF5(g) + 2 IF(g) with ΔH⁰rxn = -89 kJ. The standard enthalpies of formation are: IF7(g) = -941 kJ/mol, IF5(g) = -840 kJ/mol, I2(g) = 62.42 kJ/mol.

Using the given reactions, what is the enthalpy change (ΔH°) for the reaction: 2 CO(g) + 2 H2(g) → CO2(g) + H2O(g)?

Using the provided table and the equation below, determine the heat of formation (in kJ/mol) for KClO₃. 2 KClO₃ (s) → 2 KClO₂ (s) + O₂ (g) ΔH° = 296.2 kJ/mol

What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 mL of solution having a density of 1.25 g/mL by 3.33 °C? (The specific heat of the solution is 3.74 J/g-K.)

When 1.50 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 33.10°C. If the specific heat of the solution is 4.18 J/(g °C), what is the heat absorbed by the solution?

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.