Enthalpies for different types of reactions

The video tutorial covers various types of enthalpy changes in chemical reactions, including combustion, atomization, bond enthalpy, and solution. It explains how energy is released or absorbed during these processes and provides examples such as the combustion of butane and glucose, atomization of dihydrogen, and dissolution of ionic compounds. The tutorial also discusses the concepts of bond dissociation and mean bond enthalpy, using methane as an example, and highlights the importance of these enthalpy changes in practical applications like cooking and industrial processes.

What is the standard enthalpy of combustion for 1 mole of butane?

• 2,802 kilojoules per mole

• 435 kilojoules per mole

• 1,665 kilojoules per mole

• 2,658 kilojoules per mole

Which of the following is true about combustion reactions?

• They are exothermic and release energy.

• They are only used in industrial applications.

• They are endothermic and absorb energy.

• They do not involve energy changes.

What is the enthalpy of atomization for dihydrogen?

• 1,665 kilojoules per mole

• 108.4 kilojoules per mole

• 435 kilojoules per mole

• 242 kilojoules per mole

In the atomization of sodium, what is the enthalpy change equal to?

• Mean bond enthalpy

• Enthalpy of sublimation

• Bond dissociation enthalpy

• Lattice enthalpy

What is the bond dissociation enthalpy of the H-H bond in dihydrogen?

• 347 kilojoules per mole

• 435 kilojoules per mole

• 428 kilojoules per mole

• 242 kilojoules per mole

How is the mean bond enthalpy of a C-H bond in methane calculated?

• By dividing the enthalpy of atomization by 4

• By adding the enthalpy of atomization and bond dissociation enthalpy

• By multiplying the enthalpy of atomization by 4

• By dividing the total enthalpy by 2

What is the formula to calculate the standard enthalpy of reaction?

• Sum of bond enthalpies of products minus reactants

• Sum of bond enthalpies of reactants minus products

• Sum of enthalpies of formation of reactants

• Sum of enthalpies of formation of products

What happens to the solubility of most salts as temperature increases?

• It increases

• It becomes zero

• It remains the same

• It decreases

What is the enthalpy of solution determined by?

• Sublimation enthalpy and dissociation enthalpy

• Combustion enthalpy and reaction enthalpy

• Bond enthalpy and atomization enthalpy

• Lattice enthalpy and hydration enthalpy

Why are fluorides generally less soluble than chlorides?

• Higher lattice enthalpy

• Lower hydration enthalpy

• Higher bond enthalpy

• Lower atomization enthalpy