BIOCHEM - Enzyme Flashcards
organic catalysts where their main function is to speed up metabolic functions in the body.
Enzymes
reaction formula for enzyme
A + B ⇌ P+ Q
formula for forward reaction
A + B to P+Q
formula for backward reaction
P + Q to A+B
symbol is used to denote an equilibrium;
means the forward reaction is equivalent to backward reaction.
⇌
what does A + B ⇌ P+ Q mean
There’s no net of formation of either A+B and P+Q; hence, they are in equilibrium.
symbol used to denote a net forward reaction.
→
formula that shows The predominant is the forward reaction or the formation of P+Q.
A+B → P+Q
portion of the total energy in the system that is available for work
Free energy, ∆G
formula for free energy (Gibbs free)
∆G = ∆H - T∆S
∆G = ∆H - T∆S meaning:
∆G (Gibbs free) is equal to ∆H (Enthalpy) total internal energy MINUS Temperature (T) multiplied by Entropy (∆S)
“heat”, equal to the total change in the
internal energy of the system
Enthalpy, ΔH
extent of disorderliness/randomness of the
system;
becomes maximum(100%) as equilibrium (forward reaction is equal to the reverse reaction) is approached
Entropy, ΔS
∆G = 0 means
Equilibrium, no net change takes place
the forward and backward reactions are equal
“Exergonic”, spontaneous
Product of temperature and entropy is bigger than enthalpy. It gives off energy
∆G ‹ 0 (negative)
“Endergonic”, nonspontaneous
Takes in energy
∆G › 0 (positive)
The downhill movement of the ball is considered ___________ because the starting ball would have a higher energy compared to the end ball.
spontaneous
the energy that must be overcome in order for the reaction to proceed
regardless if it is spontaneous (exergonic) or nonspontaneous (endergonic)
activation energy
the energy of the reactants is higher than the energy of products
exergonic (energy release)
activation energy for reaction proceeds rapidly
low activation energy
activations energy that cause slow reaction
high activation energy
between endergonic and exergonic reactions, which among the two energies of their reactants are far from the activation energy?
Endergonic, because the initial energy of the reactant in exergonic is already high enough that it only needs a small amount of energy
to reach the activation energy as compared to the endergonic reaction.
reactants are at a lower free energy level than the products
endergonic
energy of the products is lower, and the difference in the energy of reactants and products are being release
exergonic reaction