Question

please explain why for each answer in table

4.Keduced organic compounds tend to contain stored energy in C-H bonds. As a general rule, the greater the number of C-H bonds, the greater the amount of potential energy stored in the molecule. Answer cach question in the chart as it relates to the two reactions shown at the top. Be sure to explain the reasoning behind your answers. ogniwolle talo Reaction 1: CH, +20, H,O+CO, (methane) Reaction 2: 600, +6H, O CH,,O, +60, a. Is the reaction exergonic or endergonic? b. Is the reaction spontaneous? c. Is the reaction anabolic or catabolic? non lo lobom il- bubade tobo ronda d. Is AG (the change in free energy) positive or negative?

Answer 1

	Reaction - 1 CH​​​​​4​​​​ + 2O2  $\rightarrow$ H​​​​​​2O + CO​​​​​2
a. Is this reaction exergonic or endergonic?	This is a type of exergonic reaction. There are four C-H bonds (methane contains four C-H bonds) in the reactant molecules and no C-H bonds are present in the resultant molecules. This means energy is released to the environment during the reaction. This is why this reaction is a type of exergonic reaction.
b. Is this reaction spontaneous?	Yes, this reaction is a spontaneous reaction. In this reaction, the potential internal energy of the reactant molecules is higher than the resultant molecules, which means this reaction does not need any external energy from the environment to occur. This is why this is a spontaneous reaction.
c. Is the reaction anabolic or catabolic?	This is a catabolic reaction. In catabolic reaction, the potential internal energy is higher in the reactant molecules than the resultant molecules. In reaction 1, the stored potential energy is higher in reactant molecules than the resultant molecules, due to the presence of more number of C-H bonds. So, this reaction is a catabolic reaction.
d. Is $\Delta$ G (the change in free energy) positive or negative?	Delta G = free energy stored in the resultant molecules - free energy stored in the reactant molecules In this reaction, the free energy stored in the resultant molecules is lower than the reactant molecules. Hence, delta G is positive in this reaction.

	Reaction - 2 6CO2 + 6H2O $\rightarrow$ C6H12O6 + 6O2
a. Is this reaction exergonic or endergonic?	This is a type of endergonic reaction. The number of C-H bonds is higher in the resultant molecules (7 C-H bonds are present in the ring structure of glucose) than the reactant molecules (0 number of C-H bonds are present in reactant molecules). This means this reaction is a type of endergonic reaction.
b. Is the reaction spontaneous?	No, this is not a spontaneous reaction. The potential energy stored in the reactant molecules is lower than the resultant molecules. This means this reaction needs energy supply from the environment to occur (in photosynthesis, sunlight is an external energy supply). So, this reaction can't take place on its own. This is why this reaction is not a spontaneous reaction.
c. Is the reaction anabolic or catabolic?	This is a catabolic reaction. In catabolic reaction, energy is stored by forming a greater number of bonds in the resultant molecules. According to the general rule, the greater the number of C-H bonds, the greater the amount of potential energy stored in the molecule, it can be said that the resultant molecules (7 C-H bonds) contain more stored potential energy than the reactant molecules (0 C-H bonds).
d. Is $\Delta$ G (the change in free energy) positive or negative?	Delta G = free energy stored in the resultant molecules - free energy stored in the reactant molecules In this reaction, the free energy stored in the resultant molecules is higher than the reactant molecules. Hence, delta G is positive in this reaction.