When 5.60 g of solid sodium reacts with excess fluorine gas to form sodium fluoride, 13.8 kJ of heat is evolved at standard state conditions. What is the standard enthalpy of formation (ΔH⁰f in kJ/mol) of solid sodium fluoride?

Using the information below, calculate the enthalpy change (ΔH°rxn) for the following reaction: CH4 (g) + 4 Cl2 (g) → CCl4 (g) + 4 HCl (g). Given the standard enthalpy of formation (ΔHf°) values: CH4 (g) = -75 kJ/mol, CCl4 (g) = -96 kJ/mol, and HCl (g) = -92 kJ/mol.

What is the total change in enthalpy when 25.0 g of solid ethanol (C2H5OH) at -125 °C is converted to liquid ethanol at -80 °C? The table below provides physical and thermochemical data for ethanol. Normal melting point: -114 °C. Assume the specific heat capacities and enthalpy of fusion are known.

What is the standard enthalpy change (∆Hrxn) for the reaction 2 CHCl3(l) → 2 C(s) + H2(g) + 3 Cl2(g) given the standard enthalpy of formation of CHCl3(l) is -134.1 kJ/mol?

When 2.275 g of anthracene, C14H10, is combusted in a bomb calorimeter with a water jacket containing 500.0 g of water, the temperature of the water increases by 43.15°C. Assuming the specific heat of water is 4.18 J/(g°C), and that the calorimeter absorbs no heat, what is the enthalpy change (ΔH) for the combustion of anthracene in kJ/mol?

Which equation represents the standard enthalpy of formation, ΔH°f, for CHCl3(l)?

Which equation represents the standard enthalpy of formation, ΔH⦵f, for CHCl3(l)?

Given the reaction 2H2 (g) + O2 (g) → 2H2O (l), which of the following is the standard enthalpy change of formation (ΔH_f) for water (H2O) in its liquid state?

Using the bond energies in Table 7.2 of your textbook, calculate the approximate enthalpy change for the following reaction: 2 H3C - CH3(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g). What is the enthalpy change?