Exergonic reactions release energy; therefore, the energy of products is lower than that of the reactants. Endergonic reactions consume energy; therefore, the energy of products is greater than that of the reactants. In other words, exergonic reactions are spontaneous, while endergonic reactions are nonspontaneous, and require the net input of energy to drive the reaction.

Exergonic reactions release energy; therefore, the energy of products is lower than that of the reactants. Endergonic reactions consume energy; therefore, the energy of products is greater than that of the reactants. In other words, exergonic reactions are spontaneous, while endergonic reactions are nonspontaneous, and require the net input of energy to drive the reaction.

A bomb calorimeter is a device used to measure the quantity of heat change for a process. The heat of a reaction which is denoted as , is the negative of the thermal energy gained by the calorimeter:

The heat capacity of a calorimeter is:

Plugging the values given into the equation gives:

Using the relation provided earlier:

Because we are dealing with 1.1 grams of sucrose, the heat of combustion of sucrose is:

A bomb calorimeter is a device used to measure the quantity of heat change for a process. The heat of a reaction which is denoted as q, is the negative of the thermal energy gained by the calorimeter:

The heat capacity of a calorimeter is:

Plugging the values given into the equation gives:

Using the relation provided earlier:

Because we are dealing with 1.65 grams of sucrose, the heat of combustion of sucrose is:

A bomb calorimeter is a device used to measure the quantity of heat change for a process. The heat of a reaction which is denoted as q, is the negative of the thermal energy gained by the calorimeter:

The heat capacity of a calorimeter is:

Plugging the values given into the equation gives:

Using the relation provided earlier:

Because we are dealing with 1.65 grams of sucrose, the heat of combustion of sucrose is:

A bomb calorimeter is a device used to measure the quantity of heat change for a process. The heat of a reaction which is denoted as , is the negative of the thermal energy gained by the calorimeter:

The heat capacity of a calorimeter is:

Plugging the values given into the equation gives:

Using the relation provided earlier:

Because we are dealing with 1.1 grams of sucrose, the heat of combustion of sucrose is:

Endothermic processes involve a positive change in enthalpy. This means that the enthalpy of products is higher than the enthalpy of reactants and net heat energy is consumed. Phase changes that involve increasing the distance between particles (meaning conversion of solid to liquid (melting), liquid to gas (evaporation) and solid to gas (sublimation)) require an input of energy and are considered endothermic processes. On the other hand, phase changes that decrease the distance between particles (such as gas to liquid (condensation), liquid to solid (freezing), and gas to solid (deposition)) release energy and are considered exothermic processes.

We need to use the following equation to answer this question:

Above, is change in Gibbs free energy, is change in enthalpy, is temperature, and is change in entropy. The question states that the reaction is spontaneous; therefore, is negative. We can also determine the for this reaction by looking at the phases of the products and reactants. Recall that entropy is a measure of disorder. When it comes to phases, gases have the highest entropy and solids have the lowest entropy. This is because in gases the molecules are spread out and have more room for disorder while solids are compressed and well packaged, decreasing the disorder of the atoms/molecules. Liquids are intermediate in entropy. In this reaction, we are creating a liquid from two molecules of gas; therefore, we are decreasing the entropy of the system (going to a more ordered, liquid state). The change in entropy for this reaction is negative.

Rearranging and solving the equation above for gives us:

Since both and are negative, will always be negative (regardless of temperature). This is an exothermic reaction.

We need to use the following equation to answer this question:

Above, is change in Gibbs free energy, is change in enthalpy, is temperature, and is change in entropy. The question states that the reaction is spontaneous; therefore, is negative. We can also determine the for this reaction by looking at the phases of the products and reactants. Recall that entropy is a measure of disorder. When it comes to phases, gases have the highest entropy and solids have the lowest entropy. This is because in gases the molecules are spread out and have more room for disorder while solids are compressed and well packaged, decreasing the disorder of the atoms/molecules. Liquids are intermediate in entropy. In this reaction, we are creating a liquid from two molecules of gas; therefore, we are decreasing the entropy of the system (going to a more ordered, liquid state). The change in entropy for this reaction is negative.

Rearranging and solving the equation above for gives us:

Since both and are negative, will always be negative (regardless of temperature). This is an exothermic reaction.

Endothermic processes involve a positive change in enthalpy. This means that the enthalpy of products is higher than the enthalpy of reactants and net heat energy is consumed. Phase changes that involve increasing the distance between particles (meaning conversion of solid to liquid (melting), liquid to gas (evaporation) and solid to gas (sublimation)) require an input of energy and are considered endothermic processes. On the other hand, phase changes that decrease the distance between particles (such as gas to liquid (condensation), liquid to solid (freezing), and gas to solid (deposition)) release energy and are considered exothermic processes.