Consider the malate dehydrogenase reaction from the citric acid cycle. Given the listed concentrations, calculate the free energy change for this reaction at energy change for this reaction at 37.0 ∘ C 37.0 ∘C (310 K). Δ G ∘ ′ ΔG∘′ for the reaction is + 29.7 kJ/mol +29.7 kJ/mol . Assume that the reaction occurs at pH 7. [malate] = 1.25 mM [malate]=1.25 mM [oxaloacetate] = 0.260 mM [oxaloacetate]=0.260 mM [NAD + ] = 270 mM [NAD+]=270 mM [NADH] = 110 mM

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%

a polar bond is formed when electrons are shared unevenly between atoms

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.