Consider the following system at equilibrium where K = 9.52x10-2 and AH° = 18.8 kJ/mol at 350 K. ? CH4 (g) + CCl4 (g) 2 CH₂Cl₂ (g) The production of CH₂Cl₂ (g) is favored by: Indicate True (T) or False (F) for each of the following: 1. increasing the temperature. 2. decreasing the pressure (by

Consider the following system at equilibrium where K = 9.52x10-2 and AH° = 18.8 kJ/mol at 350 K. ? CH4 (g) + CCl4 (g) 2 CH₂Cl₂ (g) The production of CH₂Cl₂ (g) is favored by: Indicate True (T) or False (F) for each of the following: 1. increasing the temperature. 2. decreasing the pressure (by

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...

See similar textbooks

Similar questions

Consider the following system at equilibrium where H° = -111 kJ/mol, and Kc = 0.159, at 723 K. N2(g) + 3H2(g) 2NH3(g) If the TEMPERATURE on the equilibrium system is suddenly decreased: The value of Kc fill in the blank 1 A. increases. B. decreases. C. remains the same. The value of Q 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 reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The concentration of H2 will: fill in the blank 4 A. increase. B. decrease. C. remain the same.
Consider the equilibrium system described by the chemical reaction below. For this reaction, Kp: 109 at 298 K. If the equilibrium partial pressures of Br2 and NOBR at 0.0159 atm and 0.0768 atm, respectively, determine the partial pressure of NO at equilibrium... %D 2 NO(g) + Br2(g) = 2 NOBr(g) 1 NEXT へ If (x) represents the equilibrium partial pressure of NO, set up the equilibrium expression for Kp to solve for the partial pressure. Do not combine or simplify terms.. Kp 109 %3D RESET (109) (0.0159) (0.0768) 2(0.0159) 2(0.0768) (0.0159)? (0.0768)² (x) (2x) (x)? (2x)?
Consider the following system at equilibrium where K. = 9.52x102 and AH° = 18.8 kJ/mol at 350 K. CH4 (g) + CC14 (g) =2 CH,Ch (g) The production of CH,Cl2 (g) is favored by: Indicate True (T) or False (F) for each of the following: |1. decreasing the temperature. | 2. increasing the pressure (by changing the volume). | 3. decreasing the volume. v 4. adding CH,Cl . | 5. removing CCI4 .
Consider the following system at equilibrium where K. = 77.5 and AH° = -108 kJ/mol at 600 K. co (g) + Cl2 (g) = COCI2 (g) The production of COCI, (g) is favored by: Indicate True (I)_or False (E) for each of the following: 1. decreasing the temperature. v 2. increasing the pressure (by changing the volume). 3. decreasing the volume. v 4. removing COCI2 . v 5. removing Cl2 .
Kc = 0.76 at a given temperature for the reaction: 2 HI (g) = H2 (g) + l2 (g) . Consider the condition [HI] = 0.36 M and [H2] = [12] = 0.60 M. Which of the following statements is correct? a) The quotient Q > Kc. b) The reaction will shift to right to establish equilibrium. O a) only O b) only Both a) and b) are correct. neither a) nor b) is correct.
2
Consider the following system at equilibrium where AH = 268 kJ and Kc = 5.10 × 10-6, at 548 K. NH4Cl(s) NH3(g) + HCl(9) The production of NH3(g) is favored by (indicate true or false): decreasing the temperature: decreasing the pressure (by changing the volume): increasing the volume: adding NH4Cl: adding HCl:
Consider the following equilibrium: N₂(g) + 3H₂(g) 2NH, (g) AG=-34. kl Now suppose a reaction vessel is filled with 3.40 atm of hydrogen (H₂) and 8.20 atm of ammonia (NH,) at 814. "C. Answer the following questions about this system: Under these conditions, will the pressure of H₂ tend to rise or fall? Is it possible to reverse this tendency by adding N₂¹ In other words, If you said the pressure of H₂ will tend to rise, can that be changed to a tendency to fall by adding Ny? Similarly, if you said the pressure of Hy will tend to fall, can that be changed to a tendency to rise by adding N₂7 If you said the tendency can be reversed in the second question, calculate the minimum pressure of N, needed to reverse it. Round your answer to 2 significant digits. Orie fall O yes Ono 7 p X 5 OG F# S
Consider the following reaction:COCl2(g) CO(g) + Cl2(g)If 2.98×10-2 moles of COCl2, 0.206 moles of CO, and 0.304 moles of Cl2 are at equilibrium in a 17.8 L container at 672 K, the value of the equilibrium constant, Kp, is .
The following reaction is at equilibrium: X(s) + 2Y(g) ⇒ 3 Z(g) Kp is 25.5 at 1500 K (R = 0.0821 L.atm/mol.K) a) Ke equation is b) An (gas) = c) Kc is calculated to be >
2. Explain how each of the following factors affects the amount of hydrogen gas present in an equilibrium mixture in the following reaction: 3 Fe(s) + 4 H,O(g) Fe;O4(s) + 4 H,(g) AH = - 150kJ a) raising the temperature of the mixture b) introducing more steam c) increasing the pressure
Consider the following system at equilibrium where AH° = -18.8 kJ, and K. = 10.5, at 350 K: %3D 2CH,Cl,(g)CHĄ(g) + CCl(g) If the TEMPERATURE on the equilibrium system is suddenly decreased: The value of K. |A. Increases B. Decreases C. Remains the same |A. Is greater than K. B. Is equal to K. C. Is less than K. The value of Q. 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 CC14 will: A. Increase. B. Decrease. C. Remain the same.