At a particular temperature the following system is at equilibrium in a closed container: 2NOCI(g) 2 2NO(g) + Cl2(g) Analysis of the equilibrium mixture shows it to have the following composition: PNOCI = PNO = 1.35x10-2 atm PCI, = 0.215 atm = 1.25 atm Calculate the value of K, for this system at this temperature. Kp = %3D Numeric input field

At a particular temperature the following system is at equilibrium in a closed container: 2NOCI(g) 2 2NO(g) + Cl2(g) Analysis of the equilibrium mixture shows it to have the following composition: PNOCI = PNO = 1.35x10-2 atm PCI, = 0.215 atm = 1.25 atm Calculate the value of K, for this system at this temperature. Kp = %3D Numeric input field

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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eaching and lea x . OWLV2 | Assignment | Finished * OWLV2 | Online teaching and lea x + enow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-take The equilibrium constant, K, for the following reaction is 55.6 at 698 K. H2 (g) + I2 (g)=2 HI (g) Calculate the equilibrium concentrations of reactants and product when 0.285 moles of H, and 0.285 moles of I, are introduced into a 1.00 L vessel at 698 K. [H2] = | [L] =| M M [HI] = M Submit Answer Retry Entire Group 9 more group attempts remaining Previous 9:53 AI 10/14/20 Inort sc fio 12 delete home en num backspace 8 lock 远

Express the equilibrium constant for the following reaction: 2 NH,(g) = N,(g) + 3 H,(g) Select one: pl/2(NH3) а. К, P(N2) × P1/3(H2) p2(NH3) b. Kp = P(N2) × P3(H2) %3D c. Kp = P(N2) » P3(H2) p2(NH3) %3D P(N2) × P1/3(H2) pl/2(NH3) d. Kp = p6(NH3) e. Kp = IN2P[H2P е. Кр
Step 4: Plug the equilibrium expressions into the equation for K and solve for x. [OH Jeq[NH4*Jeq Kb = [NH3Jeg = x² 2 1.2 - X Equation 15.30 x² 1.2-X +² Because K₁ 4.6 x 10-³ M = Equation 15.32 1.8 x 10-5 Remember, when K is on the borderline value of ≈10-5, it's a good habit to check and see if x < 5% of the initial concentration of the original molecule. .. assumption is valid K 7 Open in
For items 10-12. The decomposition of NH4Cl (s) at a given temperature of 548 K, the Kp = 0.01072. NH4Cl (s) = NH4 (g) + HCl (g) 10. If 10.00 g of solid NH4Cl (s) is introduced to the reaction vessel of 500 mL and the system is allowed to reach equilibrium, calculate for the partial pressure of the ammonia. NH4Cl (s) NH4 (g) + HCl (g) C. 0.0212 atm A. 0.104 atm B. 8.41 atm D. 5.30 atm E. 0.00198 atm 11. What is the Kc of the reaction at the given temperature? A. 2.48 x 10-⁹ B. 2.35 x 10-4 C. 1.59 x 10-3 D. 5.16 x 10-6 12. Calculate the temperature needed to change the Kp of the reaction to twice of the initial equilibrium constant. The A,H= 176.01 kJ/mol A. 538 K B. 558 K C. 265 K D. 285 K
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For the reaction A + B --> 2 C, Kç = 0.16. A 2.00 L flask is filled with 1.00 mol A and 1.00 mol B, and allowed to come to equilibrium. Determine the concentrations, in moles/liter, of A, B and C at equilibrium. (Do not input units, 3 sig figs). A = B = C =
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A chemist at a pharmaceutical company is measuring equilibriumconstants for reactions in which drug candidatemolecules bind to a protein involved in cancer. The drugmolecules bind the protein in a 1:1 ratio to form a drug–proteincomplex. The protein concentration in aqueous solutionat 25 °C is 1.50 x 10-6 M. Drug A is introduced into the proteinsolution at an initial concentration of 2.00 x 10-6 M.Drug B is introduced into a separate, identical protein solutionat an initial concentration of 2.00x 10-6 M. At equilibrium,the drug A–protein solution has an A–protein complexconcentration of 1.00 x 10-6 M, and the drug B solutionhas a B–protein complex concentration of 1.40 x 10-6 M.Calculate the Kc value for the A–protein binding reactionand for the B–protein binding reaction. Assuming that thedrug that binds more strongly will be more effective, whichdrug is the better choice for further research?
For items 10-12. The decomposition of NH4C1 (s) at a given temperature of 548 K, the Kp = 0.01072. NHẠCI (s) =NH4 (g) + HCl (g) 10. If 10.00 g of solid NH4C1 (s) is introduced to the reaction vessel of 500 mL and the system is allowed to reach equilibrium, calculate for the partial pressure of the ammonia. NHẠCI (s) = NH4 (g) + HCl (g) C. 0.0212 atm A. 0.104 atm B. 8.41 atm D. 5.30 atm E. 0.00198 atm 11. What is the Kc of the reaction at the given temperature? C. 1.59 x 10-3 A. 2.48 x 10-9 B. 2.35 x 10-4 D. 5.16 x 10-6 12. Calculate the temperature needed to change the Kp of the reaction to twice of the initial equilibrium constant. The A,H = 176.01 kJ/mol A. 538 K B. 558 K C. 265 K D. 285 K