At what temperature (if any) is this reaction endergonic? 1,3-Bisphosphoglycerate + ADP →ATP + 3-Phosphoglycerate + H+: AH = 41.02 kJ/mol and AS = 0.3030 kJ/molk. Report your answer in Kelvin using inequality signs with out and extra spaces added in. For example T=100.00K T>100.00K T<100.00K T/=100.00K greater than or equal to type your answer...

17. Given the following set of reaction data, AH = -285.83 kJ mol- H2 (g)+}02(8) 2B(s) +3H, (8) 2B(s) +O2(8) –→ B,O3(s) → H2O(1) → B,H, (8) AH = 36.4 kJ mol- AH = –1273.5 kJ mol determine the heat of reaction (in kJ mol') for the following reaction. – B2O3 (s) +3H,0(1) w bns maldorg B,H, (8) + 30, (g) - AH = ? kJ mol-1 lo teari done roi noltaupa 189T) of 9je s beau mo A: –2167

Coupling Endergonic & Exergonic Reactions in Metabolism (Hess's Law). Use the appropriate AG°ʻ values below from the table. You have to pick the correct two equations in the table to obtain the desired equation (the hydrolysis of acetyl-CoA) below. Reaction AG° (kJ/mol) Oxaloacetate + acetyl-CoA + H20 → citrate + COASH + H* Malate → fumarate + H20 -32.2 3.8 Oxaloacetate + acetate → citrate -0.8 Malate + NAD* → oxaloacetate + NADH + H+ 29.7 Oxaloacetate + 2H* + 2e¯ → malate?- -32.04 Using the informațion in the table above, calculate AG" for the following reaction (the hydrolysis of acetyl-CoA): Acetyl-CoA + H2O → Acetate + COASH + H* AG" = ? 0.16 kJ/mol -28.4 kJ/mol -61.9 kJ/mol 31.4 kJ/mol 64.24 kJ/mol -64.24 kJ/mol -2.5 kJ/mol 28.4 kJ/mol -31.4 kJ/mol 61.9 kJ/mol -33.0 kJ/mol 2.5 kJ/mol -31.54 kJ/mol 36.0 kJ/mol 33.0 kJ/mol -0.16 kJ/mol 31.54 kJ/mol -36.0 kJ/mol OO O O O 000 0 00000 O000

For the aqueous reaction CH2OH キャーキャ H-C-OH CH2- dihydroxyacetone phosphate glyceraldehyde-3-phosphate the standard change in Gibbs free energy is AG°' = 7.53 kJ/mol. Calculate AG for this reaction at 298 K when [dihydroxyacetone phosphate] = 0.100 M and [glyceraldehyde-3-phosphate] = 0.00600 M. AG= kJ/mol

21. Given the following two equations CH5OH(1) + 3 O2(8) 2 СO2(g) + 3 Н20(1) AH = -1370 kJ С-Н(8) + 3 О2(s) → 2 CO2(g) + 2 H2O(1) AH = -1410 kJ Calculate AH for the reaction C2H4(8) + H2O(1) CH5OH(I) ΔΗ- a. -2780 kJ b. 2780 kJ с. 40 kJ d. 40 kJ

Given that the reaction of 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 3 H20 (g) ΔΗ - - 906 kJ What would AH for NO (g) + ? H20 (g) → NH3 (g) + O2 (g) be? 2. 906 kJ 226.5 kJ -226.5kJ 453 kJ

At what temperature (if any) is this reaction exergonic?   1,3-Bisphosphoglycerate + ADP →ATP + 3-Phosphoglycerate + H+: ΔH = 41.02 kJ/mol and   ΔS  = 0.3030  kJ/molK.  Report your answer in Kelvin using inequality signs with out and extra spaces added in. For example T=100.00K T>100.00K T<100.00K T</=100.00K  less than or equal to  T>/=100.00K  greater than or equal to

Consider the following reactions: 3C(s)+4H,(g)→C;H,(g) AH° =-103.8kJ C(s)+0,(g)→ CO,(g) AH° =-393.5kJ %3D H,(g)+-0,(g)→H,O(g) AH' =-241.8kJ %3D 2 What is AH in kJ for the overall reaction? C3H&(g) + 502(g) → 3CO2(g) + 4H2O(g)

Energy from ATP hydrolysis drives many nonspontaneouscell reactions:AT P⁴⁻(aq) +H₂O(l) ⇌ADP³⁻(aq) +HPO₄²⁻(aq) +H(aq) ΔG°'=-30.5 kJ Energy for the reverse process comes ultimately from glucose metabolism:C₆H₁₂O₆(s)+ 6O₂g) →6CO₂(g) +6H₂O(l)(a) Find K for the hydrolysis of ATP at 37°C.(b) Find ΔG'°ᵣₙₓ for metabolism of 1 mol of glucose. (c) How many moles of ATP can be produced by metabolism of1 mol of glucose? (d) If 36 mol of ATP is formed, what is the actual yield?

Calculate the standard free-energy change of the reaction catalysed by the enzyme phosphoglucomutase Glucose-1-P =Glucose-6-P, given that, starting with 21.54 mM Glucose-1-P and no Glucose-6-P, the final equilibrium mixture at 25°C and pH=7.0 contains 10.34 mM Glucose-6-P and the remaining Glucose-1-P. Give the answer in J/mol.K to one decimal place. You may find these constants useful: Physical constants and Units Used in Thermodynamics (link opens in new page)