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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
- 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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