1) When you increase the temperature in a system, enzymes have a habit of denaturing. Explain what is happening in relation to the Gibbs Free Energy Equation: ΔG = ΔH – TΔS. Remember, in order to maintain a highly ordered system, energy needs to be used for maintenance. If the free energy decreases, then spontaneous reactions occur. First Define: ΔG: ΔH: ΔS: T: Explain:

Explanation:

When enzyme is denatured due to high temperature the reaction slows down because enzymes are catalyst that speeds up rate of reaction hence , the gibbs free energy which is energy at work reduces due a decrease in enzymatic reaction that affects the overall reaction.

ΔG = ΔH - TΔS

Gibbs free energy is the energy at work i.e the energy that use to do work

Gibbs free energy equation determines if a chemical equation is spontaneous or not. If ΔG is negative, it is spontaneous, if it is positive, it is not spontaneous.

Enthalpy is the

sum of internal heat with pressure and the volume of the system

Internal heat+pressure+ volume

ΔH is change in enthalpy, or energy in a system, and

Entropy is the rate of disorderliness of a system, when a system is highly disordered the entropy is high TΔS is difference in entropy multiplied by temperature, and entropy is the energy that is not used for work and accumulates as waste heat. So if difference in enthalpy is greater than difference in entropy multiply by temperature it means energy was added to the system.

option a and d is the correct answer

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