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201 Le Chatelier's Principle in Iron Thiocyanate Equilibrium Prelab Name. _Section , Le Chatelier's Principle in Iron Thiocyanate Equilibrium 1. Write down the equilibrium constant expression for the following reaction: Co2+(aq) + 4 Cl -(aq) = CoCl,²-(aq) In which direction will the equilibrium shift if you (a) increase the concentration of Co²* and (b) decrease the concentration of CoCl,²-? 2. Using Le Chatelier's principle, predict the direction of the net reaction in each of the following equilibrium systems, as a result of increasing the pressure at constant temperature. a. N2(g) + Oz(g) 5 2 NO(g) b. PCI5(g) = PC13(g) + Cl2(g) c. CO(g) + Cl,(g) = COC,(g) 3. What effect (shift to the right or left) does an increase in temperature have on each of the following systems at equilibrium? a. 3 0%(g) 5 203(g) AH = 284 kJ b. 2S03(g) + O2(g) = 2S03(g) AH = -198.2 kJ %3D

201 Le Chatelier's Principle in Iron Thiocyanate Equilibrium Prelab Name. _Section , Le Chatelier's Principle in Iron Thiocyanate Equilibrium 1. Write down the equilibrium constant expression for the following reaction: Co2+(aq) + 4 Cl -(aq) = CoCl,²-(aq) In which direction will the equilibrium shift if you (a) increase the concentration of Co²* and (b) decrease the concentration of CoCl,²-? 2. Using Le Chatelier's principle, predict the direction of the net reaction in each of the following equilibrium systems, as a result of increasing the pressure at constant temperature. a. N2(g) + Oz(g) 5 2 NO(g) b. PCI5(g) = PC13(g) + Cl2(g) c. CO(g) + Cl,(g) = COC,(g) 3. What effect (shift to the right or left) does an increase in temperature have on each of the following systems at equilibrium? a. 3 0%(g) 5 203(g) AH = 284 kJ b. 2S03(g) + O2(g) = 2S03(g) AH = -198.2 kJ %3D

Chemistry
Chemistry
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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
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201 Le Chatelier's Principle in Iron Thiocyanate Equilibrium Prelab Name, Section Le Chatelier's Principle in Iron Thiocyanate Equilibrium 1. Write down the equilibrium constant expression for the following reaction: Co2*(aq) + 4 Cl-(aq) = CoCl,²-(aq) In which direction will the equilibrium shift if you (a) increase the concentration of Co²+ and (b) decrease the concentration of CoCl,2-? 2. Using Le Chatelier's principle, predict the direction of the net reaction in each of the following equilibrium systems, as a result of increasing the pressure at constant temperature. a. N2(g) + O2(g) # 2 NO(g) b. PCIS(g) PC13(g) + Cl2(g) CO(g) + Cl,(g) 5 COCI,(g) C. 3. What effect (shift to the right or left) does an increase in temperature have on each of the following systems at equilibrium? a. 3 O2(g) 5 203(g) AH = 284 kJ b. 2S03(g) + O2(g) 5 2S03(g) AH = -198.2 kJ
Transcribed Image Text:201 Le Chatelier's Principle in Iron Thiocyanate Equilibrium Prelab Name, Section Le Chatelier's Principle in Iron Thiocyanate Equilibrium 1. Write down the equilibrium constant expression for the following reaction: Co2*(aq) + 4 Cl-(aq) = CoCl,²-(aq) In which direction will the equilibrium shift if you (a) increase the concentration of Co²+ and (b) decrease the concentration of CoCl,2-? 2. Using Le Chatelier's principle, predict the direction of the net reaction in each of the following equilibrium systems, as a result of increasing the pressure at constant temperature. a. N2(g) + O2(g) # 2 NO(g) b. PCIS(g) PC13(g) + Cl2(g) CO(g) + Cl,(g) 5 COCI,(g) C. 3. What effect (shift to the right or left) does an increase in temperature have on each of the following systems at equilibrium? a. 3 O2(g) 5 203(g) AH = 284 kJ b. 2S03(g) + O2(g) 5 2S03(g) AH = -198.2 kJ
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