Carbon monoxide is toxic because it bonds much more strongly to the iron in hemoglobin (Hgb) than does O 2 . Consider the following reactions and approximate standard free energy changes: Hgb + O 2 → HgbO 2 Δ G ∘ = − 70 KJ Hgb + CO → HgbCO Δ G ∘ = − 80 KJ Using these data, estimate the equilibrium constant value at 25°C for the following reaction: HgbO 2 + CO ⇌ HgbCO + O 2
Carbon monoxide is toxic because it bonds much more strongly to the iron in hemoglobin (Hgb) than does O 2 . Consider the following reactions and approximate standard free energy changes: Hgb + O 2 → HgbO 2 Δ G ∘ = − 70 KJ Hgb + CO → HgbCO Δ G ∘ = − 80 KJ Using these data, estimate the equilibrium constant value at 25°C for the following reaction: HgbO 2 + CO ⇌ HgbCO + O 2
Solution Summary: The author explains that the value of K is to be calculated at given temperature for the reaction between HgbO_
Carbon monoxide is toxic because it bonds much more strongly to the iron in hemoglobin (Hgb) than does O2. Consider the following reactions and approximate standard free energy changes:
Hgb
+
O
2
→
HgbO
2
Δ
G
∘
=
−
70
KJ
Hgb
+
CO
→
HgbCO
Δ
G
∘
=
−
80
KJ
Using these data, estimate the equilibrium constant value at 25°C for the following reaction:
Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction free energy of the following chemical reaction:
MgCl2 (s) + H2O (l) = MgO (s) + 2HCl (g)
The standard free energy of formation, DGf°, of atomic oxygen is 230.1 kJ/mol. Determine the equilibrium constant for the following reaction at standard thermodynamic conditions.
O2(g) ↔ 2O(g)
As a result of an experiment following measurements were obtained from a cell: ATP concentration of 0.5 mM, ADP concentration of 0.1 mM, inorganic phosphate (Pi) concentration of 2 mM. Under these conditions calculate the actual free energy (ΔG) of the reaction of hydrolysis of ATP to ADP and Pi. (The standard energy (ΔG°) of ATP = −31 kJ/mol; RT = 2.58 kJ/mol)
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY