Construct the expression for Kp for the following reaction. CC(g) = C(s) + 2 Cl2(g) 1 Drag the tiles into the numerator or denominator to form the expression. Each reaction participant must be represented by one tile. Do not combine terms. Kp II = Pc (PCI)² PCCI RESET PCCI₁ 2(PCC) (PCC)² Pc 2(Pc) (PC)² Pcl, 2(PCI) (PCI)²

Construct the expression for Kp for the following reaction. CC(g) = C(s) + 2 Cl2(g) 1 Drag the tiles into the numerator or denominator to form the expression. Each reaction participant must be represented by one tile. Do not combine terms. Kp II = Pc (PCI)² PCCI RESET PCCI₁ 2(PCC) (PCC)² Pc 2(Pc) (PC)² Pcl, 2(PCI) (PCI)²

Introductory Chemistry: A Foundation

8th Edition

ISBN:9781285199030

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 20QAP

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Distinguish between the terms equilibrium constant and reaction quotient. When Q = K, what does this say about a reaction? When Q K, what does this say about a reaction? When Q K. what does this say about a reaction?
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For the reaction N2(g)+3H2(g)2NH3(g) show that Kc = Kp(RT)2 Do not use the formula Kp = Kc(RT)5n given in the text. Start from the fact that Pi = [i]RT, where Pi is the partial pressure of substance i and [i] is its molar concentration. Substitute into Kc.
For which reactions in Exercise 34 is Kp equal to K?
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
Nitrosyl chloride, NOC1, decomposes to NO and Cl2 at high temperatures. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) Suppose you place 2.00 mol NOC1 in a 1.00–L flask, seal it, and raise the temperature to 462 °C. When equilibrium has been established, 0.66 mol NO is present. Calculate the equilibrium constant Kc for the decomposition reaction from these data.
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