Step-by-step explanation:
We have to consider the following reaction:
CH₃CH₂OH + 3 O₂ ----> 2 CO₂ + 3 H₂O ΔH = -1,235 kJ/mol
a) What type of reaction is this?
This a combustion reaction, it is an exothermic reaction also (since ΔH is negative, that means that heat is released)
b) If more CH₃CH₂OH is added to the system, how will the reactions shift to reach the equilibrium again?
When adding a reactant to a reaction that is at equilibrium, the reaciton will shift to the right. The reaction will try to consume the additional reactant that was added and more and more products will be produced.
c) If water is extracted from the system, how will the reactions shift to reach the equilibrium again?
The reactions will shift to the right. The reactions will try to produce more water in order to replace the water that is being extracted.
d) If heat is removed from the system, how will the reactions shift to reach the equilibrium again?
Since we said before that this is an exothermic reaction and heat is being released we can assume that heat is a product and rewrite the equation like this.
CH₃CH₂OH + 3 O₂ ----> 2 CO₂ + 3 H₂O + Q
In this case we are in the same scenario that in the previous question. A product is being removed from the system, so the reaction will shift to the right in order to return to the equilibrium.
e) What is the name of the principle that helps you predict each of these shifts in equilibrium?
Le Châtelier's principle.
Answer:
a) combustion reaction, exothermic reaction.
b) will shift to the right.
c) will shift to the right.
d) will shift to the right.
e) Le Châtelier's principle.