The pka of H₂O is 15.7, and the pKa of NH4* is 9.24. Do you think the reaction mixture at equilibrium will contain: A) Mostly products B Mostly reactants Equal amounts of both
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- AH = - 1.2 kcal/mol; Kp = 16 nM OH 1 НО AH = - 6.0 kcal/mol; Kp = = 76 nM OH HOllio AH = - 5.5 kcal/mol; Kp = 0.5 nM OH 3 (ii) What is the significance of Kp? Hence, arrange the three molecules in terms of decreasing affinity to their target. O=3) One of the main buffer systems found in living organisms is the phosphate buffer system, often used in biological research to mimic cellular conditions. The phosphate equilibrium reactions and their corresponding pKa's are as follows: H3PO4 = H* + H2PO, H2PO, = H+ + HPO?- HPO- = H+ + PO;- pKa1 pКаz —D 7.21 = 12.44 = 2.12 pKa3 (a) Given the above chemical reaction, write out the expression for K, of the buffer system which would predominate at neutral pH conditions. Justify your choice. (b) The human body, and many other lifeforms, prefer an internal pH of 7.2 to maintain homeostasis. However, some more acid-tolerant or basic-tolerant organisms can survive (and sometimes thrive) within different ranges of pH. Calculate the mass and moles of the correct acid and corresponding conjugate base solid (assume you have sodium salts of each base: NaH,PO4, Na,HPO4, and Na PO,) which are needed to make 500 mL of a 0.5 M buffer solution (0.5 M total, including the concentration of acid and base…For the reaction - what effect would adding large amounts of heat have on the equilibrium? (Which way would it shift and why?) Explain in terms of LeChatelier’s Principle. Fe3O4(s) + 4 H2 (g) <_-> 3 Fe (s)+ 4 H2O (g) ΔH = 36 kcal Keq = 2.3 x 10-18 During the process of ketogenesis in the liver, 3-hydroxybutyric acid and acetoacetic acid are in equilibrium with each other. However, acetoacetic acid can decompose to form carbon dioxide and acetone in a nonreversible reaction. Answer the following by using LeChatelier’s Principle. What effect would the nonreversible decomposition of acetoacetic acid have on the equilibrium between 3-hydroxybutyric acid and acetoacetic acid? (i.e. which way would if shift?) What effect would the nonreversible decomposition of acetoacetic acid have on the concentration of 3-hydroxybutric acid? (i.e. would it go up or down)
- 4 NH3(g) + 5 O2 >>><<<4 NO(g) + 6 H2O(g) + 126 kcal Which way will the equilibrium shift and what will be ghe effect on the concentration of the NO if the concentration of the ammonia is increased? Decreased?On the basis of Kc for the following reaction, would you expect the reaction to go almost completely to product at equilibrium? 2SO2(g) + O2(g) ↔ 2SO3(g); Kc = 3x1025 Yes No On the basis of Kc for the following reaction, would you expect nearly complete reaction at equilibrium? 2HF(g) ↔ 2H2(g) + F2(g); Kc = 3x10-95 Yes NoConsider the following equation: 2SO2(g)+O2(g)=2SO3(g). At 700 0C, a 500mL reaction vessel contains 1.20*10-3 mol of SO2, 5.0*10-4 mol of O2 and 1.0*10-4 mol of SO3. (a) If Kc is 1.7*106 at 700 0C, will the reaction favor the formation of more products or reactants? (b) what are the equlibrium concentrations of the products and reactants?
- For the reaction: PC15(g) + heat <> PCI3(g) + CI2 (g). How will the following affect the equilibrium? a) Reduction of PCI5, b) Increase in pressure, c) Removal of heat, d) Addition of CI2Given the reaction: 4 NH39) + 5 O2(g) 4 NOG) + 6 H20O Determine AG° Will the reaction go spontaneously? No 241.4 kcal -241.4 kcal ||-214.4 kcal YesLe Châtelier’s principle is related ultimately to the rates ofthe forward and reverse steps in a reaction. Explain (a) why anincrease in reactant concentration shifts the equilibrium positionto the right but does not change K; (b) why a decrease in Vshiftsthe equilibrium position toward fewer moles of gas but does notchange K; (c) why a rise in Tshifts the equilibrium position of anexothermic reaction toward reactants and also changes K;and(d) why a rise in temperature of an endothermic reaction from T1to T₂ results in K₂ being larger than K1
- Part A A person who has been a smoker and has a low oxygen blood saturation uses an oxygen tank for supplemental oxygen. The following equation depicts oxygen binding with hemoglobin: What is the stress on the equilibrium of the reaction between oxygen and hemoglobin? Hb(aq) + O2(g)= HbO2(aq) O The oxygen concentration is decreased. Answer the following questions to describe what happens when oxygen is first supplied. O The oxygen concentration is increased. O The HbO2 concentration is decreased. The hemoglobin concentration is increased. In what direction does the hemoglobin equilibrium shift? O The equilibrium shifts in the direction of the reactants. O The equilibrium shifts in the direction of the products. O The equilibrium does not change.C=a4bc46ac4 Part A X Given the two reactions 1. H₂S(aq) = HS (aq) + H+ (aq), K₁=9.46x10-8, and 2. HS- (aq) = S²-(aq) + H+ (aq), K2 = 1.31x10-19, what is the equilibrium constant Kfinal for the following reaction? DO Enter your answer numerically. ► View Available Hint(s) Kfinal Submit W LIVE ΑΣΦ MacR Pearson Education Inc. All rights reserved. Terms of Use | Privacy Policy | Permissions Contact Us D P Pearson zoom S² (aq) + 2H+ (aq) = H₂S(aq) t O ? ReviewWhat does the K value tell you about reactions and how do you know if the reactants are more stable than the products?