Enthalpy Changes of Reactions

What type of reaction is shown in the reaction pathway?

• endothermic reaction

• exothermic reaction

Tags

NGSS.HS-PS1-4

C+ O₂ --> CO₂ + 60kJ, what is the value for ΔH for the reaction?

• +60

• -60

• there is no way to know

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

What will ΔH be if there is 1 mole of oxygen?

• -500 kJ

• 500 kJ

• -750 kJ

• -4500 kJ

Tags

NGSS.HS-PS1-4

What mass of P₄ must be reacted to produce 5905 kJ of energy?

• 25.43 g

• 563.0 g

• 2.421 g

• 300.0 g

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1

2N₂ + 3H₂ --> 2NH₃ + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?

• 92 kJ

• 0.143 kJ

• 23 kJ

• 15 kJ

Tags

NGSS.HS-PS1-4

The term "enthalpy" in the context of chemical reactions refers to:

• The total kinetic energy of the reactants

• The heat content of a system at constant pressure

• The electrical energy produced by the reaction

• The amount of light emitted by the reaction

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

What type of reaction is this?

• Exothermic

• Endothermic

• Kinetic

• Potential

Tags

NGSS.HS-PS1-4

In an endothermic reaction, the energy of the products is:

• Lower than the energy of the reactants.

• Higher than the energy of the reactants.

• Equal to the energy of the reactants.

• Unrelated to the energy of the reactants.

Tags

NGSS.HS-PS1-4

The bond formation in chemical reactions is generally:

• Endothermic

• Exothermic

• Neither endothermic nor exothermic

• Both endothermic and exothermic, depending on the reaction

Tags

NGSS.HS-PS1-4

What is required for an endothermic reaction to proceed?

• Release of energy

• Absorption of energy

• Decrease in temperature

• Increase in pressure

Tags

NGSS.HS-PS1-4