The Gibbs free energy change of a reaction can be calculated using the equation ΔG = ΔH – TΔS. A biochemical reaction that can p
rovide energy for cellular metabolism would be one in which: Choose one: A. ΔG was negative. B. all terms on the right are negative. C. ΔG was positive. D. all terms on the right are positive.
The answer is a. ΔG was negative because, for a biochemical reaction to occur and provide energy for cellular metabolism, the Gibbs free energy ΔG = ΔH - TΔS < 0 , for spontaneity. If all terms on the right were to be negative, then ΔG = -ΔH - (-TΔS) = TΔS - ΔH and would only be less than zero if the absolute value of ΔH > absolute value of TΔS. If ΔG was positive as in C, the reaction would not be spontaneous and energy would have to be put into the biochemical reaction for it to occur. If all terms on the right were positive, then, ΔG = ΔH - TΔS < 0 when TΔS > ΔH , else ΔG > 0 and energy would have to be put into the biochemical reaction for it to occur, so its not spontaneous.
The answer is B the water is being heated so the molecules are bouncing around and then the energy is released increasing kinetic energy and decreasing potential energy
