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- Prove that statement mathematically?3) The enzyme aldolase catalyzes the conversion of fructose-1,6-diphosphate (FDP)to dihydroxyacetone phosphate (DHAP) and glyceraldehide-3-phosphate (G3P). Thereaction isFDP ⇄ DHAP + G3P , ∆rG0(298.15 K) = 23.8 kJ mol−1In red blood cells the concentration of these species are [FDP] = 35 µM, [DHAP] =130 µM, and [G3P] = 15 µM. (Remember that 1.0 µM = 1.0 × 10−6 mol L−1. Thestandard state for reactions in solution can be taken as c0 = 1.0 mol L−1).Calculate ∆rG in a red blood cell at 25 0C. Will the reaction occur spontaneouslyin the cell at this temperature?Hydrogen is one of only seven elements which exist as stable diatomic molecules at (or close to) room temperature and atmospheric pressure. Let’s investigate just how much more thermodynamically favorable diatomic hydrogen is compared to atomic hydrogen. Given the following reaction and associated data at T = 298.15 K. 2 H(g) ⇌ H"(g) or equivalently H(g) + H(g) ⇌ H2(g) Δf?° (kJ mol-1) ?° (kJ K-1 mol-1) H(g) 218.0 0.115 H2(g) 0 0.131 Calculate ΔH, ΔS, and ΔG for the formation of H2(g) from H(g) at 298.15 K. Calculate KP for the reaction. Calculate the temperature at which the reverse reaction becomes favorable. Assume ΔH and ΔS do not change with temperature.
- 3. A particular protein heat denatures with a melting temperature Tm = 332 K with an enthalpy of unfolding, AHm = 372 kJmol-¹. (a) What is the entropy of unfolding in kJ mol-1 K-1 at Tm? (b) If ACp is 6.6 kJ mol-1 K-1, at what temperature does the free energy of unfolding (AG unfolding) have the greatest value (i.e. the native state is most stable)? (c) Calculate the value of AG and K at this temperature.5. One might imagine that a reluctant pair of Diels-Alder reactants (diene and dienophile) could eventually be forced to react in high conversion by increasing the temperature. What might prevent the higher temperature from getting the job done. Think about the equation DG = DH - TDS. What the heck is entropy?Consider a molecule having three energy levels as Part A follows: What is the probability that this molecule will be in the lowest-energy state? State Energy (cm-1) Degeneracy Express your answer to three significant figures. 1 1 500. 3 ΑΣφ 3 1500. 5 Imagine a collection of N molecules all at 400. K in which one of these molecules is selected. Pi = Note: k = 0.69503476 cm¬1 . K-1. Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
- An experiment involving inorganic syntheses of molecular precursors to organometallic ceramics requires reactions that involve the formation of a metal-metal bond. The percentage of such a bond forming is p=20% If X is the number of successful reactions out of 25 such experiments; a) what is the minimum number of successful reactions are formed if 58% of them form the metal-metal bond? b) what is the probability of having the third successful reaction on the 5th experiment? c) What is the probability that the successful bond is formed for the first time on the 3th experiment?A student determines the value of the equilibrium constant to be 55.2 for the following reaction. C2H4(g) + H,O(g)- →CH;CH2OH(g) Based on this value of Keqi AG° for this reaction is expected to be (greater,less) than zero. Calculate the free energy change for the reaction of 1.64 moles of C,H.(g) at standard conditions at 298K. kJ rxnP2C.4 From the following data, determine A,H° for diborane, B,H,(g), at 298 K: (1) B,H,(g) + 30,(g) → B,O,(s) +3 H,O(g) A̟H° =-1941kJ mol -> %3D (2) 2B(s) + 를0,(g) → B,O, (s) A̟H® =-2368 kJ mol (3) H,(g)+±O,(g) → H,O(g) A,H° =-241.8kJ mol %3D
- [References] Use the References to access important values if needed for this question. A student determines the value of the equilibrium constant to be 1.54 x 1025 for the following reaction. CO(g) + 3H₂(g) → CH4 (9) + H₂O(g) Topics] Based on this value of Keq: AGO for this reaction is expected to be than zero. Calculate the free energy change for the reaction of 1.73 moles of CO(g) at standard conditions at 298 K. AGO kj rxn Submit Answer Retry Entire Group 4 more group attempts remaining2. In a non-ideal binary mixture of A and B, the chemical potential of A is (a) The partial derivative of the total Gibbs free energy, with respect to the number of moles of A. (b) The partial derivative of the Gibbs free energy of A, with respect to the number of moles of A. (c) The partial derivative of the Gibbs free energy of B, with respect to the number of moles of A. (d) The total Gibbs free energy, divided by the number of moles of A. (e) The Gibbs free energy of A, divided by the number of moles of A.Given the following data: CO(g)+H20(g)→ CO,(g)+ H2(g) AH° (25°C) = -42.0 kJmol1 C, (CO) = 26.8 + 6 x 10³T JK'mol1 C, (H2O) = 30.1+ 10 x 10³T JK'mol1 Cp (H2) = 28.5 + 2 x 10³T JK'mol1 C, (CO2) = 26.4 + 42 x 10³T JK-'mol1 where T is the thermodynamic temperature, calculate the change in enthalpy for the reaction at 1000 K.