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What happens to the equilibrium if the pressure is increased?
equilibrium will shift to the side of the equation with the least moles in attempt to reduce pressure in the haber process N2+3H2 <--> 2NH3 an increase in pressure causes equilibrium to shift the right because it has the least moles (2 instead of 4) <--> represents a reversible reaction sign
What happens of the equilibrium of a weak acid dissociation reaction were upset?
The reaction would shift to balance the change
How can a chemical reaction shift toward the desired direction?
You can make it shift, by Le Chatliers principle. Or. By Reaction Quotient method and comparing it against the Equilibrium constant.
Would happen if the equilibrium of a weak acid dissociation reaction were upset?
The reaction would shift to balance the change
How does reaction quotient predicts the direction of a reaction?
The reaction quotient is the ratio of products to reactants not at equilibrium. If the system is at equilibrium then Q becomes Keq the equilibrium constant. Q = products/reactants If Q < Keq then there are more reactants then products so the system must shift toward the products to achieve equilibrium. If Q > Keq then there are more products than reactants and the system must shift toward the reactants to reach equilibrium.
If the reaction gets hot is it an endothermic or an exothermic reaction?
The reverse reaction is not always endothermic or exothermic, the reverse reaction is the opposite of whatever the initial reaction is, so if the reaction is endothermic, the reverse reaction is exothermic and vise versa.
How will increasing the temperature affect the equilibrium?
It depends if the reaction is exothermic or endothermic. For example: If the reaction requires energy (endothermic), then energy (i.e. 100kJ) will be a reactant on the left-hand side. Then, use Le Chatelier's Principle from there. If you increase the temperature of the system in equilibrium, it will shift towards the product/right-hand side. If you decrease the temperature of the system, it will shift towards the reactants/left-hand side.
What happens to the equilibrium if the pressure is increased?
equilibrium will shift to the side of the equation with the least moles in attempt to reduce pressure in the haber process N2+3H2 <--> 2NH3 an increase in pressure causes equilibrium to shift the right because it has the least moles (2 instead of 4) <--> represents a reversible reaction sign
What piece of information will tell you which way the equilibrium of a reaction will shift due to a change in temperature?
The enthalpy of the reaction.
What would happen if the equilibrium of a weak dissociation reaction were upset?
The reaction would shift to balance the change
What happens of the equilibrium of a weak acid dissociation reaction were upset?
The reaction would shift to balance the change
What effect does the removal of heat have on the equilibrium position?
The temperature of a reaction will entirely change th equilibrium position for any given reaction. If I'm right, as you increase the temperature, the equilibrium shifts closer to the endothermic reaction as there is more heat to consume. It may also, of course, change other properties of the substances involved in the reaction, but that depends on the chemicals.
A reaction that gives out energy?
... is an exothermic reaction (opposite of 'endothermic')
A reaction that releases energy in the form of heat?
It is called an exothermic reaction. Example: a burning candle
How can a chemical reaction shift toward the desired direction?
You can make it shift, by Le Chatliers principle. Or. By Reaction Quotient method and comparing it against the Equilibrium constant.
What would happen if the equilibrium of a weak acid dissociation reaction were upset?
The reaction would shift to balance the change
Would happen if the equilibrium of a weak acid dissociation reaction were upset?
The reaction would shift to balance the change
