Calculate the enthalpy change for the reaction: NO(g) + O(g) -> NO2(g), given the following standard enthalpies of formation: ΔHf°[NO(g)] = 90.25 kJ/mol, ΔHf°[O(g)] = 249.17 kJ/mol, ΔHf°[NO2(g)] = 33.18 kJ/mol.

A 0.1326 g sample of magnesium was burned in an oxygen bomb calorimeter. The total heat capacity of the calorimeter plus water was 5,760 J/°C. If the temperature rise of the calorimeter with water was 0.570°C, calculate the enthalpy of combustion of magnesium in kJ/mol.

What is the enthalpy change (ΔH) for the dissolution of 1 mole of substance X in water, given that the temperature of the solution increases from 12.0 °C to 30.0 °C when 1.40 g of X is dissolved in 35.0 mL of water? Assume the specific heat capacity of water is 4.18 J/g°C and the density of water is 1.00 g/mL.

Which of the following expressions correctly calculates the change in enthalpy (ΔH) for a reaction using standard heats of formation?

Which of the following statements is true regarding the enthalpy change of a reaction when the quantities of reactants are doubled?

Calculate the standard enthalpy change for the following reaction at 25°C using the standard enthalpies of formation: C3H8 (g) + 5O2 (g) -> 3CO2 (g) + 4H2O (g). Given: ΔHf° [C3H8 (g)] = -104.7 kJ/mol, ΔHf° [CO2 (g)] = -393.5 kJ/mol, ΔHf° [H2O (g)] = -241.8 kJ/mol.

Choose the reaction that illustrates the standard enthalpy of formation (ΔHf°) for Ca(NO2)2.

Which of the following reactions represents the standard enthalpy of formation (ΔHₒƒ) for CsHSO4(s)?

Consider the combination reaction: 2Mg(s) + O2(g) → 2MgO(s) with ΔH = -1204 kJ. What is the enthalpy change for the decomposition of 1 mole of MgO(s) into Mg(s) and O2(g)?