Consider the following reaction where Ke = 10.5 at 350 K: 2 CH2CI2 (g) = CH4 (g) + CCI4 (g) A reaction mixture was found to contain 1.05x10 2 moles of CH2CI2 (g), 2.23x10 2 moles of CH4 (g), and 3.60x10-2 moles of CCI4 (g), in a 1.00 liter container. Indicate True (I) or False (E) for each of the following: v 1. In order to reach equilibrium CH2CI2(g) must be consumed v 2. In order to reach equilibrium Ke must decrease. v 3. In order to reach equilibrium CH4 must be consumed. v 4. Qç is greater than Kc. v 5. The reaction is at equilibrium. No further reaction will occur.

Consider the following reaction where Ke = 10.5 at 350 K: 2 CH2CI2 (g) = CH4 (g) + CCI4 (g) A reaction mixture was found to contain 1.05x10 2 moles of CH2CI2 (g), 2.23x10 2 moles of CH4 (g), and 3.60x10-2 moles of CCI4 (g), in a 1.00 liter container. Indicate True (I) or False (E) for each of the following: v 1. In order to reach equilibrium CH2CI2(g) must be consumed v 2. In order to reach equilibrium Ke must decrease. v 3. In order to reach equilibrium CH4 must be consumed. v 4. Qç is greater than Kc. v 5. The reaction is at equilibrium. No further reaction will occur.

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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Consider the following reaction that has a Kc = 2.4 x 10^-3 at 1000K: N2(g) + 3 H2(g) = 2NH3(g) in a reaction vessel that is 5.0 x 10^3 L, 250 moles of N2, 250 mol of H2, and 50.0 mol of NH3 are mixed. write the reaction quotient. Calculate Qc.
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Consider the following reaction where Kc = 1.20×10-2 at 500 K:PCl5 (g) PCl3 (g) + Cl2 (g)A reaction mixture was found to contain 0.115 moles of PCl5 (g), 4.47×10-2 moles of PCl3 (g), and 4.16×10-2 moles of Cl2 (g), in a 1.00 liter container.Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium PCl5(g) must be consumed . 2. In order to reach equilibrium Kc must increase . 3. In order to reach equilibrium PCl3 must be consumed . 4. Qc is less than Kc. 5. The reaction is at equilibrium. No further reaction will occur.
Consider the following reaction where Ke = 9.52x10 at 350 K. CHa(9) + CCla(0) =2CH,Cl2(9) A reaction mixture was found to contain 3.07x102 moles of CHa(g), 3.96x10 moles of CCIA(g) and 1.21x102 moles of CH,Cl2(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, Qo 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.
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As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°C