study of uie gas phase at 400 K NOCI(g)- →NO(g) + % Cl2(g) the following data were obtained: NOCI], M seconds 5.08x10-2 2.54x10-2 3.75x104 1.27x10-2 1.13×105 6.35x10-3 2.63×105 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 5.08×10-2 M is Mis Js and when the starting concentration is 2.54×10-2 (2) The average A(1/[NOCI]) / At from t= 0 s to t = 3.75×104 s is The average A(1/[NOCI]) / At from t= 3.75x104 s to t = 1.13×10° s is (3) Based on these data, the rate constant for this order reaction is

study of uie gas phase at 400 K NOCI(g)- →NO(g) + % Cl2(g) the following data were obtained: NOCI], M seconds 5.08x10-2 2.54x10-2 3.75x104 1.27x10-2 1.13×105 6.35x10-3 2.63×105 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 5.08×10-2 M is Mis Js and when the starting concentration is 2.54×10-2 (2) The average A(1/[NOCI]) / At from t= 0 s to t = 3.75×104 s is The average A(1/[NOCI]) / At from t= 3.75x104 s to t = 1.13×10° s is (3) Based on these data, the rate constant for this order reaction is

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Multiply both sides of the equation by the same expression: (Be sure that the answer field changes from light yellow to dark yellow before releasing your answer.) x (In[A] – In [A],) = x(-kt) Drag and drop your selection from the following list to complete the answer: 1 -k k k k
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6. For the reaction Cu(s) = Cu(g) AH° = 81,730 – 0.47T – 0.731x10³T² AS° = 34.94 – 1.08 log1,T – 1.46 x 10³T www Set up the expression for AG° as a function of T.
Consider the following reaction where Kc CO(g) + Cl₂(g) CoCl₂(g) = 77.5 at 600 K: A reaction mixture was found to contain 4.16×10-² moles of CO(g), 4.43×10-² moles of Cl₂(g) and 0.106 moles of COCl₂(g), in a 1.00 Liter container. Indicate True (T) or False (F) for each of the following: TF 1. In order to reach equilibrium COCI₂(g) must be consumed. 2. In order to reach equilibrium Kċ must decrease. 3. In order to reach equilibrium CO must be consumed. 4. Qc is greater than Kc. 5. The reaction is at equilibrium. No further reaction will occur.
Consider the reaction SO, Ch(g) S0, (g) + Ca(g) K-2.97 x 10 at 62s K In a reaction mbture at equilibrium, the partial pressure of SO, is 141 mbar and that of Cla ln 283 mbar Part A What is the partial pressure of SO, Cl,? Express your answer in bars to three significant figures. > View Available Hint(s) V AZ * O a ? bar P(SO,Cl) = Submit Besuest Answer Next>
إغلاق ...) (1501130 General chemistry 1 section2) 0.09 Hydrogen (H2), less dense than oxygen (02), .7 5: diffuses )1 نقطة( times as fast 1/16 times fast 16 times fast 4 times fast 1/4 CO(g) + 2H2(g) =CH3OH KP = 0.038.8 What is the value of Kc for the reaction at 200 C( %3D 5 R=0.0821 atm.L/mol.K)
In which of the following processes is AH = AU? Two moles of hydrogen iodide gas react to form hydrogen gas and iodine gas in a 40-L container. O Calcium carbonate is heated to form calcium oxide and carbon dioxide in a container with variable volume. One mole of solid carbon dioxide sublimes to the gas phase. O One gram of water is vaporized at 100°C and 1 atm. O Two moles of ammonia gas are cooled from 325°C to 300°C at 1.2 atm
6. Consider the following reaction: CO(g) + H2O(g) CO2(g) + H2(g) Ko = 0.58 at 1273 K* A sealed 4.00L vessel initially contains 1.00 mole CO2(g), 1.00 mole H2(g), 0.600 moles CO(g), and 0.600 moles of H2O(g). Calculate the moles of H2(g) present at equilibrium. The NG Reference: General Chemistry 8th Ed: Ebbing and Gammon: 2005 by Houghton Mifflin. New York. page 654, print 68
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (The system is considered in equilibrium if Kc and Qc are within 5% of each other.) (a.) 2 SO3(g) 2 SO2(g) + O2(g) Pi(SO3) = 0.100 atm, Pi(SO2) = 1.10 atm, Pi(O2) = 1.20 atm, Kp = 5.5 atm What is the reaction quotient? What direction will the reaction shift to? LEFT or RIGHT? (b.) 2 NO(g) + Cl2(g) 2 NOCl(g) Pi(NO) = 1.25 atm, Pi(Cl2) = 1.25 atm, Pi(NOCl) = 0 atm, Kp = 3.1 ✕ 103 What is the reaction quotient? What direction will the reaction shift to? LEFT or RIGHT? (c.) N2(g) + O2(g) 2 NO(g) [N2]i = 0.120 M, [O2]i = 0.240 M, [NO]i = 1.20 M, Kc = 0.050 What is the reaction quotient? What direction will the reaction shift to? LEFT or RIGHT?
Question 15 of 16 Submit Consider the reaction below: 2 SO3(g) =2 SO2(g) + O2(g) The Kp is 1.81 × 10-5 at 350.0°C. Calculate Kc at the same temperature. (R = 0.08314 L·bar/ mol · K.) 1 2 3 4 C 7 8 9 +/- х 100 Tap here or pull up for additional resources LO
The salt ammonium nitrate can follow three modes of decomposition: (a) to HNO; (g) and NH3(g), (b) to N₂O(g) and H₂O(g), and (c) to N₂ (g), O2 (g) and H₂O(g). Calculate AGixn for each mode of decomposition at 298 K. Compound AG NH3(g) -16.4 NH4NO3(s) -183.9 HNO3(g) -73.5 N₂O(g) 103.7 H₂O(g) -228.6 (kJ/mol) (b) to N₂O(g) and H₂O(g) Express your answer kilojoules per mole to one decimal place. AGIX = Submit Part C AGix= IT ΑΣΦ A Submit Request Answer (c) to N₂ (g), O₂(g), and H₂O(g) Express your answer in kilojoules per mole to one decimal place. | ΑΣΦ A ? Request Answer kJ/mol ? kJ/mol