In the uncatalyzed reaction N₂O₂(g) = 2 NO₂ (s) at 100 °C, the pressure of the gases at equilibrium are present? D the system will shift from left to right the system will shift from right to left the system will shift from left to right no effect N₂O4 = 0.377 atm and PNO₂ = 1.56 atm. What would happen to these pressures if a catalyst were

In the uncatalyzed reaction N₂O₂(g) = 2 NO₂ (s) at 100 °C, the pressure of the gases at equilibrium are present? D the system will shift from left to right the system will shift from right to left the system will shift from left to right no effect N₂O4 = 0.377 atm and PNO₂ = 1.56 atm. What would happen to these pressures if a catalyst were

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 12QAP: Write a chemical equation for an equilibrium system that would lead to the following expressions...

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When a mixture of hydrogen and bromine is maintained at normal atmospheric pressure and heated above 200. °C in a closed container, the hydrogen and bromine react to form hydrogen bromide and a gas-phase equilibrium is established. Write a balanced chemical equation for the equilibrium reaction. Use bond enthalpies from Table 6.2 ( Sec. 6-6b) to estimate the enthalpy change for the reaction. Based on your answers to parts (a) and (b), which is more important in determining the position of this equilibrium, the entropy effect or the energy effect? In which direction will the equilibrium shift as the temperature increases above 200. °C? Explain. Suppose that the pressure were increased to triple its initial value. In which direction would the equilibrium shift? Why is the equilibrium not established at room temperature?
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