Consider the v vs [s] plot. The Km for the uninhibited reaction is 8.0 6.0 Om ol min 4.0 2.0 1.0 2.0 3.0 4.0 IS] mM O05 mM O3 mM O80 mmol/miY C40mmol/min -----
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- 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?The equilibrium constant K for the reaction 2CI(g)CI2(g) was measured as a function of temperature (Kelvin). A graph of In (K) versus 1/T for this reaction gives a straight line with a slope of 1.352 104 K and a y-intercept of 14.5 1. Determine the values of H and S for this reaction. See Exercise 79.A chemical engineering student is studying the effect of pH on the corrosion of iron. Ellie following data are collected: Corrosion Rate (mm/year) ph 0.03 13.00 0.06 12.00 0.16 11.00 0.22 10.00 0.25 9.00 0.25 8.00 0.25 7.00 0.25 6.00 0.25 5.00 0.27 4.00 0.37 3.00 0.38 2.80 0.63 2.80 1.00 2.80 Plot corrosion rate vs. pH. (HINT: Label the x axis with decreasing pH.) (a) How would you describe the dependence of corrosion on pH? (b) When the pH goes below 3, bubbles appear in the solution. What change takes place in the reduction half-reaction at low pH? (c) How do you explain the shape of the curve at the lowest pH? (Based on a graph in the Kirk-Otbmer Encyclopedia of Chemical Technology, 4th ed., vol 7. New York: John Wiley & Sons, p. 559.)
- A 51.0-LL reactor at 1600 KK is charged with 50.0 gg of NiO(s)NiO(s) and 1.40 atmatm of CO(g)CO(g). After equilibrium is reached, what is the partial pressure of CO2(g)CO2(g) in the reactor?Predict the spontaneity of this reaction at standard state but the concentration of HCl is 12.0M. MnO2(s) + 4H+ + 2Cl- ----> Mn2+ + Cl2 (g) + 2H2 O Can we get Cl2 by this reaction at the given condition?At 25oC, for the reaction 2 A(aq) ----> B(aq) + C(aq), the equilibrium constant is 1.79 . If the concentration of B(aq) were 0.311 M and the concentration of C(aq) were 0.477 M, what would be the minimum concentration of A(aq) required (in mol/L) to make this reaction spontaneous under these conditions?
- At 25oC, for the reaction 2 A(aq) ----> B(aq) + C(aq), the equilibrium constant is 1.89. If the concentration of B(aq) was 0.361 M and the concentration of C(aq) was 0.496 M, what would be the minimum concentration of A(aq) necessary in order (in mol/L) to make this reaction spontaneous under these conditions?The equilibium constants of the reactions FeO(s) + CO(g) = Fe(s) + CO2(g) ; K1 FeO (s) + H2(g) = Fe(s) + H2O (g) ; K2 Temp (oC) 600 700 800 900 1000 ------------------------------------------- K1 0.900 0.673 0.535 0.453 0.396 K2 0.332 0.422 0.499 0.594 0.668 Calculate the Equilibium constant of the reaction CO (g) + H2O (g) = CO2(g) + H2(g) at the above temperature Also calculate the heat of the reaction for the production of hydrogen from carbon monoxide and water vapour, assuming it to be independent of temperatureFor the following reaction: A(g) + 3 B(g) ⇌ C(g) + 2 D(g) Calculate the magnitude of Kp (don't report the units) assuming the following composition at equilibrium: PA = 0.61 bar PB = 0.926 bar PC = 0.24 bar PD = 0.779 bar
- A student measures the reaction H2(g) + Cl2(g) <=> 2 HCl(g) concentrations at a few different temperatures and obtains the equilibrium constant. The student wants to use the van't Hoff equation to roughly determine the reaction enthalpy assuming that it does not change over the region of interest. T (K) 300 500 1000 Keq 4×1031 4×1018 4×108 So the student plots the data in the lnK vs 1/T diagram and obtains a linear fitting shown below: What is the reaction enthalpy value obtain from this figure? __________ kJ/mol. 3sig fig. (hint, rearrange the equation so that you can clearly see the slop and the intercept. )The following questions refer to the following reaction at constant 25°C and 1 atm.2Fe(s) + (3/2)O2(g) + 3H2O(l) 2Fe(OH)3(s) H = –789 kJ/molSubstance S° (J/mol K)Fe(OH)3(s) 107Fe(s) 27O2(g) 205H2O(l) 70a. Determine Ssurr for the reaction (in kJ/mol K)b. Determine Suniv for the reaction (in kJ/mol K)2.65c. What is the G for this reaction?d. Calculate the equilibrium constantAt 25oC, the equilibrium constant for the reaction 2 A(aq) ----> B(aq) + C(aq) is 1.99 . If the concentration of B(aq) is 0.366 M and the concentration of C(aq) is 0.460 M, what would be the minimal concentration of A(aq) (in mol/L) required to make the reaction spontaneous?