Consider the following system at equilibrium where AH° = -16.1 k), and Kc = 154 , at 298 K: 2 NO (g) + Br2 (g) =2 NOB (g) If the TEMPERATURE on the equilibrium system is suddenly decreased : The value of Kc A. Increases B. Decreases C. Remains the same The value of Qc A. Is greater than Kc B. Is equal to K. C. Is less than Kc The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of Br2 will: A. Increase. B. Decrease. C. Remain the same.

Consider the following system at equilibrium where AH° = -16.1 k), and Kc = 154 , at 298 K: 2 NO (g) + Br2 (g) =2 NOB (g) If the TEMPERATURE on the equilibrium system is suddenly decreased : The value of Kc A. Increases B. Decreases C. Remains the same The value of Qc A. Is greater than Kc B. Is equal to K. C. Is less than Kc The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of Br2 will: A. Increase. B. Decrease. C. Remain the same.

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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Consider the following system at equilibrium where AH° = -16.1 kJ, and K, = 154 , at 298 K: 2 NO (g) + Br2 (g) :2 NOB (g) If the TEMPERATURE on the equilibrium system is suddenly increased : The value of K.A. Increases B. Decreases C. Remains the same The value of Q.JA. Is greater than K. B. Is equal to K, C. Is less than K. The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of Br2 will:DA. Increase. B. Decrease. C. Remain the same.
Consider the following system at equilibrium where AH° = -87.9 kJ/mol, and K. = 83.3 , at 500 K. PCI3 (g) + Cl2 (g) = PCI5 (g) When 0.22 moles of PCI3 (g) are removed from the equilibrium system at constant temperature: The value of Ke increase. decrease. remain the same. The value of Qc K.. is greater than is equal to is less than The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. Oremain the same. It is already at equilibrium. The concentration of Cl, will increase. decrease. remain the same.
Consider the following system at equilibrium where AH° = -10.4 kJ, and K. 55.6, at 698 K. %3D H2(9) + I2(9) 2HI(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value of Ke A. increases. B. decreases. C. remains the same. The value of Qc A. is greater than Ke. B. is equal to Ke. C. is less than Ke. The reaction must: A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The number of moles of I2 will: A. increase. B. decrease, C. remain the same.
Consider the following reaction at 25oC: A2(g) + B2(g) 2 AB(g) Which of the following statements is true? A. K > 1; at equilibrium there is more products than reactants. B. K > 1; at equilibrium there is more reactants than products. C. K < 1; at equilibrium there is more products than reactants. D. K < 1; at equilib thisrium there is more reactants than prroducts.
Consider the following system at equilibrium where AH° = -87.9 k), and K. = 83.3, at 500 K. PCI3(g) + Cl2(g) PCI5(g) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature: The value of K. A. increases. B. decreases. C. remains the same. The value of Qc A. is greater than Kc. B. is equal to Kc. C. is less than Kc. The reaction must: A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The number of moles of Cl, will: A. increase. B. decrease. C. remain the same.
Consider the following system at equilibrium where AH° -16.1 k), and K. = 154 , at 298 K: 2 NO (g) + Br2 (g) 2 NOBR (g) If the TEMPERATURE on the equilibrium system is suddenly increased : The value of K. A. Increases B. Decreases C. Remains the same The value of Qc A. Is greater than K. B. Is equal to Kc C. Is less than K. The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of Br2 will: A. Increase. B. Decrease. C. Remain the same.
Consider the following system at equilibrium where AH° = 10.4 kJ, and Kc = 1.80×10-2, at 698 K: 2HI(g) =H₂(g) + I₂(9) If the TEMPERATURE on the equilibrium system is suddenly decreased: The value of Kc A. Increases B. Decreases C. Remains the same The value of Qc A. Is greater than Kc B. Is equal to Kc C. Is less than Kc The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of I2 will: A. Increase. B. Decrease. C. Remain the same.
Consider the following system at equilibrium where K. 7.00x10-5 and AH° = 182 kJ/mol at 673 K. NH4I (s) = NH3 (g) + HI (g) The production of NH3 (g) is favored by: Indicate True (I) or False (F) for each of the following: 1. increasing the temperature. v 2. decreasing the pressure (by changing the volume). v 3. increasing the volume. v 4. adding NH4I . 5. removing HI .
Consider the following system at equilibrium where H° = -18.8 kJ, and Kc = 10.5, at 350 K:2CH2Cl2(g) CH4(g) + CCl4(g)If the TEMPERATURE on the equilibrium system is suddenly increased: The value of Kc fill in the blank 1 A. Increases B. Decreases C. Remains the same The value of Qc fill in the blank 2 A. Is greater than Kc B. Is equal to Kc C. Is less than Kc The reaction must: fill in the blank 3 A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of CCl4 will: fill in the blank 4 A. Increase. B. Decrease. C. Remain the same.
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8:57 Question 6 of 25 Submit Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 5.0 L reaction vessel contained a mixture of 1.2 mol CH4, 2.8 mol H2S, 0.63 mol CS2, and 0.042 mol H2 at 93.0 °C. What are the values of Kc and Kp for the reaction at this temperature? CH.(g) + 2 H;S(g) =CS2(s) + 4 H2(g) 1 2 Based on the given data, set up the expression for Kc and then evaluate it. Do not combine or simplify terms. Kc = [0.042] 5 RESET [1.2] [2.8] [0.63] [0.042] [0.24] [0.56] [0.13] [0.0084] 2[2.8] [2.8]? 2[0.56] [0.56]? 4[0.042] [0.042]* 4[0.0084] [0.0084]* 0.063 16 6.6 x 10-8 1.5 x 107 Tap here or pull up for additional resources
O b. 1 O c. 3 O d. 6 O e. 7 Consider the following equilibrium reaction: H2CO3 (aq) = H° (aq) + HCO;" (aq): K = 5.0 x 10-7 If the initial concentrations of the species are: [H,CO) = 0.100 M [H"] = 2.00 x 10-5 M [HCO,] = 2.00 x 10³ M Which one of the statements below describes the relationship between Q and K and then the correct direction of chemical change Select one: Oa Q-K so the reaction is at equilibrium. 1bQ