Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Determine the activation energy from the following data.
| Temperature (oC) | K (s-1) |
| 189.7 | 2.52x10-5 |
| 251.2 | 3.16x10-3 |
Group of answer choices
7.74 kJ/mole
158 kJ/mole
0.574 kJ/mole
19.0 kJ/mole
0.653 kJ/mole
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- A. Consider the endothermic reaction at 25oC: FeSCN+2(aq) --><-- Fe+3(aq) + SCN-(aq) What direction will the reaction shift in response to the following stresses? (Use arrows or write "right" , "left" , or "no shift"). d. The pressure of the air around the reaction is doubled. e. Solid iron (III) chloride (FeCl3) is added. B. At 25oC, Kc for thr above reaction is 9.1 x 10-6. Determine the equilibrium concentration of Fe+3 in the solution if 0.50 mol of FeSCN+2 is dissolved to make 2.50 liters of solution. Please answer question A d and e. Also question B.arrow_forwardN204(g) = 2 NO2(g) Three experiments were run starting with different initial amounts of N2O4(g) ([N204]o in the table). The systems were allowed to reach equilibrium and the concentrations for each gas were measured (in units of moles/Liter). For each of the boxes below, calculate the ratios indicated by the column heading. This will show the mathematical relationship that exists between the concentrations of NO2 and N204 at equilibrium. Be sure to round to the correct number of significant figures. Exp[N204l0 [NO2][N,04] [NO,] / [N204] 2 [NO,] / [N204] [NO2]? / [N204] 1 3.7 2.92 2.2 2 3.0 2.56 1.7 3 2.3 2.15 1.2 Based on your calculations, indicate whether each statement is True (T) or False (F): v1. Each experiment started with a different initial concentration of N204. v2. The ratio ([NO2] / [N204]) is equal to a constant value. v3. The ratio (2 [NO2] / [N204]) is equal to a constant value. v 4. The ratio ([NO2]? / [N204]) is equal to a constant value. v5. Each experiment reached a…arrow_forwardpart d and earrow_forward
- The following figure shows Arrhenius plots for four different reactions. Which reaction has the greatest temperature dependence? In k a Ob 0 d V/T darrow_forwardThe progress of the reaction H2(g) + Br2(g) 2 2 HBr(g) can be monitored visually by following changes in the color of the reaction mixture (Br2 is reddish brown, and H2 and HBr are colorless). A gas mixture is prepared at 700 K, in which 0.40 atm is the initial partial pressure of both H2 and Br, and 0.90 atm is the initial partial pressure of HBr. The color of this mixture then fades as the reaction progresses toward equilibrium. Give a condition that must be satisfied by the equilibrium constant K (for example, it must be greater than or smaller than a given number).arrow_forwardConsider the reaction: 2S (s) + 30₂ (9)2SO3(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: 3 80 For answers with both a subscript and a superscript, enter the subscript first. For example, enter K if the first equilibrium constant should be squared. K = E D S(s) + O2(g) → SO₂(g) K₁ SO₂(g) + 1/2O₂(g) SO3(9) K₂ 13 с Submit Answer $ 888 FA F4 R F Show Hint V Retry Entire Group 9 more group attempts remaining % 5 T Cengage Learning Cengage Technical Support F G 6 B MacBook Air FO Y H & 7 N F7 U J * 00 8 ➤11 FO I M ( 9 V K O < H дв ) O L F10 question. P command F11 A ; Previous { + alt #2 “ . ? option Save and Exit I 1 delete 1 ente rearrow_forward
- *****arrow_forwardThe equilibrium constant (Kp) is 0.11 at a particular temperature for the reaction: N204(9) = 2NO2(9) Given the following sets of initial conditions, what is the net change that must occur for the reaction to reach equilibrium? Does the reaction shift left to reach equilibrium, does the reaction shift right to reach equilibrium or is the reaction at equilibrium at these initial concentrations so no net change will occur? A. PNO, = 0.105 atm, PN,0, = 0.146 atm В. PNO, = 0.093 atm, PN,0, = 0.054 atm С. PNO, = 0.180 atm, PN,0, = 0.134 atm %3D D. PNO, = 0.088 atm, PN,0, = 0.07 atm Е. PNO, = 0.055 atm, PN,0, = 0.06 atm %3D %D A. right B. left C. left D. equilibrium left right E. > >arrow_forwardConsider the following equilibrium: N204(g) = 2NO2(g) Suppose two different experiments were conducted on this equilibrium, at two different temperatures. Trial Temperature Initial Moles of N204 Equilibrium Moles of N204 1 25°C 1.00 0.815 55°C 1.00 0.500 What conclusion may be drawn from the above data? O Kc> Kp at all temperatures. The reaction is exothermic. The forward reaction proceeds faster than the reverse reaction. OKp =D1 at 55°C. O The equilibrium constant increases with increasing temperature.arrow_forward
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