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1.Consider the following reaction occurring in a closed chemical system. Assume that this reaction is at equilibrium and that in general the reaction to the right is favored.
CH3CH2OH + 3O2 2CO2 + 3H2O-->∆H = –1,235 kJ/mol
• What type of chemical reaction is this?
• If more CH3CH2OH is added to the system, how will the reactions shift to reach equilibrium again?
• If water is extracted from the system, how will the reactions shift to reach equilibrium again?
• If heat is removed from the system, how will the reactions shift to reach equilibrium again?
• What is the name of the principle that helps you predict each of these shifts in equilibrium?
3. Chalcocite is an ore from which copper can be extracted for commercial use. The formula for this important ore is Cu2S. In the laboratory it is formed by the following reaction:
2Cu + S → Cu2S
The reaction takes place in laboratory conditions that allow the reactant atoms to move freely about in the reaction vessel. Explain this reaction in terms of collision theory.
CH3CH2OH + 3O2 2CO2 + 3H2O-->∆H = –1,235 kJ/mol
• What type of chemical reaction is this?
• If more CH3CH2OH is added to the system, how will the reactions shift to reach equilibrium again?
• If water is extracted from the system, how will the reactions shift to reach equilibrium again?
• If heat is removed from the system, how will the reactions shift to reach equilibrium again?
• What is the name of the principle that helps you predict each of these shifts in equilibrium?
3. Chalcocite is an ore from which copper can be extracted for commercial use. The formula for this important ore is Cu2S. In the laboratory it is formed by the following reaction:
2Cu + S → Cu2S
The reaction takes place in laboratory conditions that allow the reactant atoms to move freely about in the reaction vessel. Explain this reaction in terms of collision theory.