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- Which is (are) able to oxidize Cl - ?(a) F2(b) F -(c) Both Br2 and I2(d) Both Br - and I -#29b except NO3 it should be NO2The molecular weight of hemoglobin is 64,500 daltons (= g mol-1). A. How much oxygen can be bound per g of hemoglobin? Express the values as mL per g of hemoglobin, where mL is the volume of O2. R =0.082 L atm mol-1 oK-1, oK =273 + oC. The molar volume of O2 is given as V = nRT/P where P = 1 atm and n= 1 mol. (Hint: 1.0 mol x 0.082 L atm mol-1 oK-1 x 273.2 oK / 1 atm = 22.4 L mol-1) (Hint: The number of moles of O2 that can be bound per g of hemoglobin is 4 x the moles of Hb in 1 g). B. The blood in a person contains 15 g of hemoglobin per 100 ml blood. How much oxygen does the blood contain at 95 mm Hg if hemoglobin is 98% saturated and the solubility of O2 is 0.003 mL dL-1 mmHg-1? (Hint: Total O2 content = HbO2 + free dissolved O2) C. Suppose the venous PO2 is 40 mm Hg, and that hemoglobin is 75% saturated at this point. What is the oxygen content of venous blood? D. Suppose the cardiac output is 5 L min-1. Calculate the oxygen delivery to the tissues from B and C. (Hint: Rate of…
- Give typed full explanation A stock solution of lithium phosphate (Li3PO4, MM= 115.794361 g/mol) is prepared by dissolving 295.8 g Li3PO4 in deionized water to a final total volume of 1.000 L. Suppose a 1.000-mL aliquot is taken from this stock solution and transferred to a new container to which deionized water is added until the total volume is 50.00 mL. A new 1.000-mL aliquot is taken from this 50.00 mL solution and transferred to a third container to which deionized water is added until the total volume is 25.00 mL. Calculate the number of individual lithium ions (Li+) in the final 25.00-mL solution. Note that lithium phosphate is a strong electrolyte that completely dissociates in water (note that (aq) means the species is a solute in an aqueous solution): Li3PO4 (aq) 3 Li+ (aq) + PO43– (aq) Report your answer to two significant figures. Use scientific notation. Example: 1.0*10^23 (this notation means 1.0 1023)Excessive nutrients dumped into waterways can create “algae blooms” that rapidly consume all of the dissolved O2 and trigger production of enough H2S to create “dead zones” like the ones that exist off the coast of Denmark and in the Gulf of Mexico immediately south of the Mississippi River delta. a. Since Group 16 element substitution is a recurring theme in that Group’s chemistry –e.g., oxygen substituting for Se and Te in the production of H2Se and H2Te, respectively –maybe molecular oxygen (O2) could be bubbled into these dead zones and react with the H2S.Write out a balanced chemical equation for the reaction between H2S and O2 to form elemental sulfur (S8) as a product that would precipitate out. b. Using bond dissociation energies, calculate if this reaction would be thermodynamically favorable. c. If your answer to part (b) is “yes”, do you think that simply bubbling O2 into these waters would work? Justify your answer.Why are the carboxylic acid groups of the amino acids so much more acidic (pK a ~ 2) thana carboxylic acid such as acetic acid (pKa = 4.76)?
- keAssignment/takeCovalentActivity.do?locator=assignment-take n progress Q Search 40 eaction is Submit Answer In the following equation for a chemical reaction, the notation (s), (I), or (g) indicates whether the substance indicated is in the solid, liquid, or gaseous state. 2NO(g) + 2H₂(g) →→→ N₂(g) + 2H₂O(l) + energy Identify each of the following as a product or a reactant: NO(g) H₂0(1) H₂(g) N₂(g) When the reaction takes place energy is V2 7 L Retry Entire Group = 18 + Use the References to access important values if needed for this question. fg 0 OWLv2 | Online teaching and lear X hp 9 8 more group attempts remaining f10 MO f11 PAI + 112 G ins prt sc Ⓡ ✰ FRIEVIDUS Next> ^ @ ¹0 delete backspace home lock 5:- 5/14For photosynthesis to occur, 2801 kJ/mole of energy is required. Add the ΔH to the correct side of the equation below: 6 CO2 (g) + H2O (l) → C6H12O6 (aq) + 6 O2 (g)ACID DEPOSITION: what are the methods used to reduce the incidence of acid deposition and photochemical smog; e.g., reducing sulfur content in fuels, using catalytic converters in automobiles, smokestack scrubbers