A favorite reaction is calcite dissolution: CACO3() + Ca2+ + CO32- K, =10-8.3 %3D a) Will the solid form or dissolve as we approach a thermal vent deep in the Pacific Ocean? b) At equilibrium, what is the change in the CO32- concentration (ExpN) if the temperature increases from 5 to 20°C? Assume the [Ca2+] = 0.001 M at both temperatures. %3D

A favorite reaction is calcite dissolution: CACO3() + Ca2+ + CO32- K, =10-8.3 %3D a) Will the solid form or dissolve as we approach a thermal vent deep in the Pacific Ocean? b) At equilibrium, what is the change in the CO32- concentration (ExpN) if the temperature increases from 5 to 20°C? Assume the [Ca2+] = 0.001 M at both temperatures. %3D

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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1 Consider the following reaction at 550 °C: 2NO(g) = 02(g) + N2(g) The equilibrium concentrations of NO, 02 and N2 are 10.6 Pa, 13.9 Pa and 11.7 Pa respectively. The Kp is 1.46. 1.1 Determine the value of Kc at 550 °C (Gas constant = 8.315 Pa m³ K-1 mol-1) 1.2 Calculate the value of K, at 1600 °C if the equilibrium concentration of 02 at 1600 °C is 4.6 Pa. 1.3 Is the forward reaction exothermic or endothermic? Give a one-sentence reason for your answer.
Given the reaction shown below: Colg) + H;0(g) CO,(g) + H2(g) K-0.640 and with the following initial concentrations: (CO)-0.626 M (CO)= 0.981 M [H,O]= 0.5 M [Ha)= 0.95 M Select the statement that best describes the reaction. O The reaction is not at equilibrium. The reaction will shift to the left to reach equilibrium. O The reaction is at equilibrium. It will not shift in either direction. O The reaction is not at equilibrium. The reaction will shift to the right to reach equilibrium. O None of these. O The reaction is not at equilibrium. The reaction will not shift on its own to reach equilibrium.
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[References] The equilibrium constant for the reaction PCl, 2 PC13 + Cl2 is 0.0245 at 250.°C. What molar concentration of PCl; would be present at equilibrium if the concentrations of PCI3 and Cl2 were both 0.161 M? Molar concentration of PCI3 = M
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A student ran the following reaction in the laboratory at 431 K: PCI 5(9) PC13(g) + Cl₂(9) When she introduced 2.02 moles of PCI5(g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂(g) to be 3.08x10-² M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
Consider the reaction N2(g) + O2(g) → 2NO(g), for which Kc = 0.81 at 300°C. Starting with initial concentrations of 0.050 M of N2 and 0.050 M of O2, set up an ICE table and determine the equilibrium concentration of NO. O (4) none given O (3) 0.100 M O (2) 0.029 M O (1) 0.015 M 3 E C 4 R F V % 5 T G 6 MacBook Pro B Y H & ∞ 7 U N * 00 8 J ۔ 9 M K O P 7
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2) For the reaction, PCI:(g) = PCl:(g) + Ch(g) at 327°C, the equilibrium constant, Ke is 0.234. Suppose that 2.082 g PCIIS is placed in an evacuated 200 mL bulb, which is then heated to 327°C. (R = 0.082 L atm mol'K', PCIS = 208.2 g/mol) (a) What would be the pressure of PCIs if it did not dissociate? (b) What is the partial pressure of PCIS at equilibrium? (c) What is the total pressure in the bulb at equilibrium? (d) What is the fraction of PCIS at cquilibrium?
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