3. When the reaction MnO (aq) + (aq) →ls)-MaOx) is balanced so that the smallest possible integers appear as stoichiometric coefficiens, the coefficient for OH" is:
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- The hydrocarbon naphthalene was frequently used in mothballs until recently, when it was discovered that human inhalation of naphthalene vapors can lead to hemolytic anemia. Naphthalene is 93.71% carbon by mass, and a 0.256-mole sample of naphthalene has a mass of 32.8 g. What is the molecular formula of naphthalene? This compound works as a pesticide in mothballs by. sublimation of the .solid so that it fumigates enclosed spaces with its vapors according to the equation Naphthalene(s)naphthalene(g)K=4.29106(at298K) If 3.00 g solid naphthalene is placed into an enclosed space with a volume of 5.00 L at 25C, what percentage of the naphthalene will have sublimed once equilibrium bas been established?What characterizes an electrolytic cell? What is an ampere? When the current applied to an electrolytic cell is multiplied by the time in seconds, what quantity is determined? How is this quantity converted to moles of electrons required? How are moles of electrons required converted to moles of metal plated out? What does plating mean? How do you predict the cathode and the anode half-reactions in an electrolytic cell? Why is the electrolysis of molten salts much easier to predict in terms of what occurs at the anode and cathode than the electrolysis of aqueous dissolved salts? What is overvoltage?3. One process for removing CO₂ from the atmosphere is to convert CO₂ to carbonate (CO3²) and then precipitate it as calcite (CaCO3). The following equilibria are relevant to this process: CO₂ (g) + 2 OH (aq) → CO32 (aq) + H₂O (1) CaCO3 (s) + 2OH- Ca(OH)2 (aq) + CO3-2 (aq) Write the K, expression for these equilibria and for the overall reaction of CO2 with Ca(OH)2.
- Calculate AH for the reaction ClF(g) + F2(g) -----> CIF3(G) from the following data: 2CIF(g) + O2(g) > Cl½0(g) + F2O(g) 2CIF3(g) + 202(g) -----> Cl½O(g) + 3F20(g) 2F2(g) + O2(g) -----> 2F2O(g) AH = 167.4 KJ --- -- AH = 341.4 KJ AH = -43.4 KJWhich reaction is most likely to have a positive ASys? a) SiO2(s) + 3 C(s) b) 6 CO2(g) + 6 H¿O(g) c) CO(g) + Cl2(g) d) 3 NO:(g) + H2O(1) 2 HN0;(1) + NO(g) SiC(s) + 2 CO(g) - CH12O6(8) + 6 O2(8) - COCI2(g)Another physiological example of an equilibrium system involves the regulation of blood pH. Carbon dioxide in the blood reacts reversibly with water to produce carbonic acid, which dissociates to produce hydronium and bicarbonate ions: CO2 (aq) + H2O (l) ⇔ H2CO3 (aq) ⇔ H3O+ (aq) + HCO3-(aq) Which of the following statement/s is/are TRUE? During strenuous exercise, the amount of carbon dioxide produced by the cells increases as a result of high metabolic activity. The increased concentration of carbon dioxide in the blood causes a shift to the right in this equilibrium to produce more carbonic acid. When this happens, the pH level of the blood increases as hydronium ion concentration increases. One of the body's responses to this imbalance in blood pH is to increase the rate of breathing so more carbon dioxide gas is exhaled from the lungs, thus shifting the equilibrium back to the left and raising the pH back to normal levels. I , II , and III I…
- 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…(Q103) Consider the formation of phosphorus pentachloride from phosphorus trichloride and chlorine gas: PCI3 (g) + Cl2 (g) PCI5 (g) If the equilibrium constant at a certain temperature is K. = 1.36, what will the equilibrium %3D concentration of PCI5 (g) be if the initial concentrations of the two reactant gases was each 0.450 M and that of the product was 0.100 M? (Note - the value of Q for the initial concentrations is 0.494, which is just a little below the value of Keg - although the reaction will proceed toward products, the final concentration of PCI5 will not increase very much).Silver chloride is classified as an insoluble compound because it dissolves only to a small extent in water. Consider the balanced equation and equilibrium constant that shows the partial dissolving of silver chloride in water: AgCl(s) = Ag*(aq) + CI"(ag) Keg = 1.70 x 10-10 a) The reaction AgCl(s) = Ag*(aq) + Cl (ag) is classified as a (homogeneous or heterogeneous) equilibrium because it involves more than one physical state, solid and aqueous. b) Based on the equilibrium constant value and the equilibrium constant expression, the concentration of each ion in a saturated solution of silver chloride is : Concentration of Ag = x 10 Concentration of CI" = x 10 M
- A sparingly soluble salt silver phosphate, Ag3PO4, is in equilibrium with its ions in solution according to the following equation A93PO4(s) = 3 Ag*(aq) + PO (aq) Write an expression for Ksp of Ag;PO4 The solubility of silver phosphate, Ag;PO4, at 25°C is 1.59 x 10 mol/L. What is the Ksp for the silver phosphate at 25°C?Write the expression for the solubility product constant for PbI2 CO (g) + 3 H2 (g) CH4 (g) + H2O (g).(a) If the molar solubility of Nd₂(CO3)3 at 25 °C is 1.00e-07 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found that 8.90e-06 g of Y₂(CO3)3 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility- product constant for Y₂(CO3)3. Ksp = (c) The Ksp of Ag₂C₂04 at 25 °C is 5.40e-12. What is the molar solubility of Ag2C₂04? solubility mol/L