SubmitPart 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 0.25 M Br2, 0.40 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 Avallable Hint(s)O 3.0 x 10-2, the reaction system proceeds to the leftO 1.1 x 10, the reaction system is at equilibriumO 0.9 x 10-4, the reaction system proceeds to the right.9 x 10-4, the reaction system proceeds to the leftSubmitPart C Complete previous part(s)< Return to AssignmentProvide FeedbackMacBook Air

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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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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
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 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 1.3 x 10 4, the reaction system proceeds to the left O 1.1 x 104, the reaction system is at equilibrium O 1.3 x 104, the reaction system proceeds to the right Submit Part C Complete previous part(s) Next > Provide Feedback MacBook Air
Consider the hypothetical reaction A(g) 2B(g). A flask is charged with 0.74 atm of pure A. after which it is allowed to reach equilibrium at 0 °C. At equilibrium the partial pressure of A is 0.37 atm Part A What is the total pressure in the flask at equilibrium? Express your answer using two significant figures. VS ΑΣΦ 4 P₁ = Submit Part B What is the value of Kp? Express your answer using two significant figures. K₂= Submit Part C Request Answer |VL ΑΣΦ Submit Request Answer What could we do to maximize the yield of B? → Request Answer [w] ? O Doing the reaction in a larger flask maximizes the yield of B. O Doing the reaction in a smaller flask maximizes the yield of B. atm
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
3 A + 2B 1 C Calculate the equilibrium constant (K) for the following reaction at 1000. K, using this information: A and B are placed in a flask and at the beginning of the reaction [A] is 6.87 M and [B] is 6.38 M. After the reaction has reached equilibrium, [C] is 1.47 M. Unfortunately, significant figures cannot be taken into account here, so please ignore them this time. 119.84085 0.00132 0.00011 0.03354 0.00834 1 1 1
Consider the following reaction at 400°C and its equilibrium constant: 2 HI(g) - 12(g) + H2(g) Kc = 0.0156 A reaction mixture contains 0.420M I2, 0.420 M H, and 3.36 M HI. Which of the following statements is TRUE? The reaction will shift in the direction of the products. The reaction quotient will decrease. The equilibrium constant will increase. OThe reaction will shift in the direction of the reactants. The system is at equilibrium.
ook at the reaction below and state which direction the reaction would shift: You remove mercury(II) oxide, HgO, from the reaction. 2HgO (s) <=> 2Hg (l) + O2 (g) Explain your reasoning
Consider the reaction below. The reaction quotient for a specific moment is 1.11. 10². If the equilibrium constant is 3.87 10², what needs to happen in order for the reaction to reach equilibria? Select all that apply. 1A+2B 3C There will be a net gain in reactant. There will be a net gain in product. The forward reaction will procede more than the reverse reaction. The reverse reaction will occur more than the forward reaction. The system will shift to the left. The system will shift to the right.
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