Question: Consider the balanced equation below the system is at equilibrium and the production of carbon dioxide and water are favored over the reverse reaction. CH

  1. Consider the balanced equation below the system is at equilibrium and the production of carbon dioxide and water are favored over the reverse reaction.

CH3CH2OH(s) + 3O2(g) 2CO2(g) + 3H2O(l) H = 1,199 kJ/mol

  • What type of chemical reaction is this (synthesis, combustion, single displacement, double displacement, decomposition or redox)? Why do you say so?
  • If more oxygen is added, how will the reactions shift to reestablish equilibrium? How do you know?
  • If water is added, how will the reactions shift to reach equilibrium again? How do you know?
  • If heat is added to this system, how will the reactions shift? How do you know?
  • Name and explain (in your own words) the principle that helps you predict each of these shifts in equilibrium.

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