Part BConsider the reaction between bromine and chlorine gases to form bromochloride:Br2 (g) + Cl2 (g)= 2BRC1(g), K. 1.11 x 10-4 at 150 KA reaction vessel contains 0.20M Br2, 0.35 M Cl2, and 3.0 x 10-3 M BrCl. Calculate the reaction quotient, Q, and determine in which direction thereaction proceeds to reach equilibrium.> View Available Hint(s)O 4.3 x 10 2, the reaction system proceeds to the leftO 1.3 x 10 4, the reaction system proceeds to the leftO 1.1 x 104, the reaction system is at equilibriumO 1.3 x 104, the reaction system proceeds to the rightSubmitPart C Complete previous part(s)Next >Provide FeedbackMacBook Air

Part B Consider the reaction between bromine and chlorine gases to form bromochloride: Br2 (g) + Cl2 (g) 2BRC1(g), K. = 1.11 x 10-4 at 150 K A reaction vessel contains 0.20M Br2, 0.35 M Cl2, and 3.0 x 10-3 M BRCI. Calculate the reaction quotient, Q, and determine in which direction the reaction proceeds to reach equilibrium. > View Avallable Hint(s) O 4.3 x 102, the reaction system proceeds to the left O 1.3 x 10-4, the reaction system proceeds to the left O 1.1 x 10, the reaction system is at equilibrium O 1.3 x 104, the reaction system proceeds to the right

Part B Consider the reaction between bromine and chlorine gases to form bromochloride: Br2 (g) + Cl2 (g) 2BRC1(g), K. = 1.11 x 10-4 at 150 K A reaction vessel contains 0.20M Br2, 0.35 M Cl2, and 3.0 x 10-3 M BRCI. Calculate the reaction quotient, Q, and determine in which direction the reaction proceeds to reach equilibrium. > View Avallable Hint(s) O 4.3 x 102, the reaction system proceeds to the left O 1.3 x 10-4, the reaction system proceeds to the left O 1.1 x 10, the reaction system is at equilibrium O 1.3 x 104, the reaction system proceeds to the right

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

Given the following reaction CO(g) + 2H₂(g) ⇒ CH₂OH(g) You have a reaction flask that contains a mixture of 0.170 M CH₂OH, 0.152 M CO, and 0.250 M H₂. Find the reaction quotient, Q, for this system. + 1 4 7 +/- 3 5 6 8 9 0 2 X C ×100
Consider an initial pressure of I2(g) of 0.100 atm in a 500 mL flask at 1000 K. With an equilibrium constant for dissociation of KP = 3.76 x 10 -3 calculate the total pressure of the system at equilibrium.
Consider the following reaction where K. = 5.10×10-6 at 548 K. NHẠCI(s)ENH3(g) + HCl(g) A reaction mixture was found to contain 5.15x10² moles of NHCI(s), 1.56×103 moles of NH3(g), and 2.26x103 moles of HCI(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.
A mixture of 0.419 M H₂O, 0.445 M CI₂O, and 0.675 M HCIO are enclosed in a vessel at 25 °C. H₂O(g) + Cl₂O(g) 2 HOCI(g) Ke=0.0900 at 25°C Calculate the equilibrium concentrations of each gas at 25 °C. [H₂O]= [CL₂O]= [HOCI]= M M M
3. Determine the reaction quotient and predict the direction that each of the following reactions will proceed to reach equilibrium: Keq = 4.6 × 10¹ a. A 1.00 L flask containing 0.0500 mol NO (g), 0.0155 mol Cl₂ (g), and 0.500 mol NOCI(g): 2NO(g) + Cl₂(g) = 2NOCI(g) A: shift right b. A 5.00 L flask containing 14 g N₂ (g), 12 g H₂ (g), and 17 g NH3(g): N₂(g) + 3H₂(g) = 2NH3(g) Keq = 0.060 (at 526 °C) c. A 2.00 L flask containing 230 g SO3 (8) 2SO3(g) = 2SO₂(g) + O₂(8) Keq = 0.230 A: shift left A: shift right
Molecular structures: The number of nonbonding electron pairs in NH3 and NH4 are 1 and 0 2 and 0 2 and 2 1 and 1 and , respectively.
Par B Consider the reaction between bromine and chlorine gases to form bromochloride: Br2(g) + Cl₂ (g) = 2BrCl(g), Kc = 1.11 x 10-4 at 150 K A reaction vessel contains 0.20 M Br2, 0.35 M Cl₂, and 3.0 x 10-3 M BrCl. Calculate the reaction quotient, Q, and determine in which direction the reaction proceeds to reach equilibrium. View Available Hint(s) O 4.3 x 10-2, the reaction system proceeds to the left O 1.1 x 104, the reaction system is at equilibrium O 1.3 x 10-4, the reaction system proceeds to the left O 1.3 x 104, the reaction system proceeds to the right Submit Review I Constants | Periodic Table P Pearson
A reaction quotient is calculated to be 3.2 x 10-5. The equilibrium constant for the same reaction is 5.4 x 10-5. Which statement is correct?
12
H2SO3 (aq) ↔ H+ (aq) + HSO3-(aq) K=1.20 x 10-2 at 25 C. There is 1.50 M of the reactant present initially. Calculate the equilibrium concentrations of all species.
Consider this equilibrium reaction at 400 K. Br, (g) + Cl, (g) = 2BRCI(g) K. = 7.0 If the composition of the reaction mixture at 400 K is [BrCl] = 0.00520 M, [Br,] = 0.00285 M, and [Cl,] is the reaction quotient, Q? = 0.000523 M, what Q = How is the reaction quotient related to the equilibrium constant, Kc, for this reaction? Q K. O Q = K.
Initially 2.6 mol CO2 and 3.4 mole H2 are placed in a 0.75 L container at 395°C. The following is the reaction equation: CO2(g) + H2(g) = CO(g) + H20(g). а. If K. = 5.67 x 10°, what are the concentrations of each substance carbon monoxide, CO, and water vapour, H2O, in the equilibrium mixture? Calculate the K, of the reaction (i) (ii)