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Suggest 4 ways in which the concentration of hydrazine, N2H4, could be increased in an equilibrium described by the following reaction N2(g) + 2H2(g) = N2H4(g) Delta H = 95 KJ

Suggest 4 ways in which the concentration of hydrazine, N2H4, could be increased in an equilibrium described by the following reaction N2(g) + 2H2(g) = N2H4(g) Delta H = 95 KJ

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Suggest 4 ways in which the concentration of hydrazine, N2H4, could be increased in an equilibrium described by the following reaction N2(g) + 2H2(g) = N2H4(g) Delta H = 95 KJ
Under what conditions will decomposition in a closed container proceed to completion so that no CaCO3 remains? 32. Explain how to recognize the conditions under which changes in volume will affect gas-phase systems at equilibrium. 33. What property of a reaction can we use to predict the effect of a change in temperature on the value of an equilibrium constant? 34. The following reaction occurs when a burner on a gas stove is lit: CH4(g) + 202(g) = CO2(g) + 2H2O(g) Is an equilibrium among CH4, O2, CO2, and H0 established under these conditions? Explain your answer. 35. A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide, SO3, from sulfur dioxide, SO2, and oxygen, O2, shown here. At high temperatures, the rate of formation of SO, is higher, but the equilibrium amount (concentration or partie' pressure) of SO3 is lower than it would be at lower temperatures. 2SO2 (g) + O2(g) = 2SO3(g) (a) Does the equilibrium constant for the reaction increase, decrease, or remain about the same as the temperature increases? (b) Is the reaction endothermic or exothermic? 36. Suggest four ways in which the concentration of hydrazine, N2H4, could be increased in an equilibrium described by the following equation: N2(g) + 2H2(g) = N¿H4(g) AH = 95 J 37. Suggest four ways in which the concentration of PH3 could be increased in an equilibrium described by the following equation: P4(g) + 6H2(g) = 4PH3(g) ΔΗ-110.5 kJ 38. How will an increase in temperature affect each of the following equilibria? How will a decrease in the volume of the reaction vessel affect each? (a) 2NH3(g) = N2(g) + 3H2(g) ΔΗ-92 kJ (b) N½(g) + O2(g) = 2NO(g) ΔΗ-181 kJ
Transcribed Image Text:Under what conditions will decomposition in a closed container proceed to completion so that no CaCO3 remains? 32. Explain how to recognize the conditions under which changes in volume will affect gas-phase systems at equilibrium. 33. What property of a reaction can we use to predict the effect of a change in temperature on the value of an equilibrium constant? 34. The following reaction occurs when a burner on a gas stove is lit: CH4(g) + 202(g) = CO2(g) + 2H2O(g) Is an equilibrium among CH4, O2, CO2, and H0 established under these conditions? Explain your answer. 35. A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide, SO3, from sulfur dioxide, SO2, and oxygen, O2, shown here. At high temperatures, the rate of formation of SO, is higher, but the equilibrium amount (concentration or partie' pressure) of SO3 is lower than it would be at lower temperatures. 2SO2 (g) + O2(g) = 2SO3(g) (a) Does the equilibrium constant for the reaction increase, decrease, or remain about the same as the temperature increases? (b) Is the reaction endothermic or exothermic? 36. Suggest four ways in which the concentration of hydrazine, N2H4, could be increased in an equilibrium described by the following equation: N2(g) + 2H2(g) = N¿H4(g) AH = 95 J 37. Suggest four ways in which the concentration of PH3 could be increased in an equilibrium described by the following equation: P4(g) + 6H2(g) = 4PH3(g) ΔΗ-110.5 kJ 38. How will an increase in temperature affect each of the following equilibria? How will a decrease in the volume of the reaction vessel affect each? (a) 2NH3(g) = N2(g) + 3H2(g) ΔΗ-92 kJ (b) N½(g) + O2(g) = 2NO(g) ΔΗ-181 kJ
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