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

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?

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?

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?

For a particular isomer of C8H18, the combustion reaction produces 5104.1 kJ of heat per mole of C8H18 consumed under standard conditions. Given that the standard enthalpies of formation for CO2(g) and H2O(l) are -393.5 kJ/mol and -285.8 kJ/mol respectively, what is the standard enthalpy of formation of this isomer of C8H18?