Endothermic and exothermic reactions Questionbank

True

False

concentration

volume

pressure

temperature

No energy is required to break bonds, and energy is only released during formation

The energy required to break bonds in the reactants is less than the energy released when forming bonds in the products

The energy required to break bonds in the reactants is greater than the energy released when forming bonds in the products

The energy required to break bonds is exactly equal to the energy released during formation

The system refers to the specific chemicals undergoing the reaction; the surroundings include everything else, such as the container and the solvent.

The system refers to the chemicals and the solvent; the surroundings include only the container and the atmosphere.

The system refers to the chemicals and the container; the surroundings include the solvent and the atmosphere.

The system refers to the container and the solvent; the surroundings include the chemicals undergoing the reaction.

Endothermic with $\Delta H = +250 \text{ kJ mol}^{-1}$

Exothermic with $\Delta H = +250 \text{ kJ mol}^{-1}$

Endothermic with $\Delta H = -250 \text{ kJ mol}^{-1}$

Exothermic with $\Delta H = -250 \text{ kJ mol}^{-1}$

True

False

$H_{\text{peak}} - H_p$

$H_r - H_p$

$H_p - H_r$

$H_{\text{peak}} - H_r$

The vertical distance from the energy of the products to the peak of the curve

The vertical distance from the energy of the reactants to the peak of the curve

The vertical distance from the energy of the reactants to the energy of the products

The vertical distance from the zero energy level to the peak of the curve

$\Delta H < 0$, endothermic

$\Delta H > 0$, exothermic

$\Delta H < 0$, exothermic

$\Delta H > 0$, endothermic

It is the energy required to reach the transition state.

It is the total heat content of the surroundings.

It is the energy released only when bonds are broken.

It is the difference between the enthalpy of the products and the enthalpy of the reactants.