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Why the reaction mixture does not have 50 percent reactant and 50 percent product at equilibrium position?
Aleenaaa
The ratio of product to reactant is dependant on many different things, from the reactants and products themselves to the pressure, temperature and other parameters of the reaction conditions such as the presence of a catalyst.
Some reactions are product favoured by nature and at room temperature and 100kPa will always lie at the product side of the equilibrium at STP. Others, like the Haber Process, are reactant favoured and, without manipulation, will produce very little product.
To maximise the product it must be made thermodynamically and entropically favourable for it to do so.
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Does a decomposition reaction decompose to a limiting reactant and a theoretical reactant?
there is a difference between decompositon reaction and to decompose the reaction mixture in (for example ice/HCl) n'mixture which for lmiting the excess reagents
Are reactants a mixture or a compound?
Reactants can be a mixture, compounds, a mixture of compounds and also elements. It depends on the reaction. Air is a mixture and is often a reactant for example.
What will happen to the reaction mixture at equilibruim if the volume of the container is increased?
The equilibrium will be re-established.
How the concentration effect the equilbrium?
The effect of the change in concentration on chemical equilibria can be predicted qualitatively by Le Chatelier's Principle. Consider the following reaction:Fe3+(aq)+SCN-(aq)Fe(SCN)2+(aq)If you add Fe3+(aq), that is an increase in the concentration of Fe3+(aq), and the equilibrium position shifts to the left (i.e. the product side). That is because the Le Chatelier's Principle states, if the reaction condition of an equilibrium system is changed, the equilibrium position will shift in a way to REDUCE the effect of the change. When the equilibrium position shifts to the left in the above system, that means the forward reaction rate increases (the backward reaction rate remains the same). More product is hence produced, in this case, Fe(SCN)2+(aq).Conversely, if you add Fe(SCN)2+(aq), the equilibrium position shifts to the right (i.e. the reactant side). This time the backward reaction rate increases while the forward reaction rate remains, hence more reactants (Fe3+(aq) and SCN-(aq)) are produced.The concentration effect on equilirium can sometimes be observed. In the above reaction, Fe3+(aq) is yellow, SCN-(aq) is colourless and Fe(SCN)2+(aq)is deep red. If the equilibrium position shifts to the left due to the concentration effect, more Fe(SCN)2+(aq) is produced and the colour of the reaction mixture becomes darker, due to the colour of Fe(SCN)2+(aq). Conversely, if the equilibrium position shifts to the right, the colour becomes paler.
Why the reaction mixture does not have 50 percent reactants and 50 percent products at equilibrium position?
At a dynamic equilibrium, a closed system of chemicals in a reversible reaction have equal rates of its forward reaction and its backward reaction. However, they may not necessarily have equal composition of its reactants and products. This is because the composition of reactants and products is governed by other factors, such as the temperature, the initial concentrations of the reactants and the stoichiometric ratios of reactants and products.Therefore, while the rates of the forward and backward reactions are equal, the composition ratios may not have to be. However, it is important to note that the concentrations of reactants and products remain constant at dynamic equilibrium. They may not be at the same concentration, but they will remain constant when an equilibrium is established.I hope this helps! :)
What does equilibrium and equilibrium mixture mean?
A quantity that characterizes the position of equilibrium for a reversible reaction; its magnitude is equal to the mass action expression at equilibrium. K varies with temperature.
Does a decomposition reaction decompose to a limiting reactant and a theoretical reactant?
there is a difference between decompositon reaction and to decompose the reaction mixture in (for example ice/HCl) n'mixture which for lmiting the excess reagents
Are reactants a mixture or a compound?
Reactants can be a mixture, compounds, a mixture of compounds and also elements. It depends on the reaction. Air is a mixture and is often a reactant for example.
What indicates a small equilibrium constant?
A small equilibrium constant value means equilibrium will never establish or the amount of products in reaction mixture is negligible.
What will happen to the reaction mixture at equilibruim if the volume of the container is increased?
The equilibrium will be re-established.
What happens if you add energy to either side of a dynamic equilibrium?
Energy is always conserved in a chemical reaction. If heat of reaction is positive, the mixture gets heated and may require external cooling to continue the reaction in the forward direction. If the reaction is endothermic, i.e. heat of reaction is negative, the mixture gets cooled and may need external supply of heat to maintain the reaction in forward direction. When the reaction is at an equilibrium, the heat of reaction is either zero or the mixture has attained an equilibrium with some definite ratios of the reaction products. The total energy of the system is conserved.
Why the reaction mixture doesn't have 50 percents reactants and 50 percents products at equilibrium position?
Chemical equilibrium occurs when the rate of the forward reaction is equal to the rate of the reverse reaction. Take this example:2NO2(g) ↔N2O4(g)At this point of the reaction the rate of N2O4 produced from NO2 is the same as the rate of NO2 produced from N2O4. The key aspect to keep in mind is that the amounts (of moles) of products and reactants at equilibrium is not always 50%/50%. It is usually not.Finding the amounts of products and reactants present during a reaction can be found using Q. Q is known as the reaction quotient. Q can be found like so:Q=[products]/[reactants]reaction quotient =concentrations of products (M) / concentrations of reactantsQ is used to find this ratio at a certain point in time during a reaction (not atequlilibrium)Most likely, you will be given Keq, the equilibrium constant, for a reaction. The value tells you the concentrations of products/reactants at equilibrium. Comparing Q and Keqwill tell you whether a reaction is at equilibrium.Not to get off topic, the answer is that equilibrium does not mean that the reaction mixture has 50% reactants and 50% products. Equilibrium means that the rate of the forward reaction equals the rate of the reverse reaction.
How the concentration effect the equilbrium?
The effect of the change in concentration on chemical equilibria can be predicted qualitatively by Le Chatelier's Principle. Consider the following reaction:Fe3+(aq)+SCN-(aq)Fe(SCN)2+(aq)If you add Fe3+(aq), that is an increase in the concentration of Fe3+(aq), and the equilibrium position shifts to the left (i.e. the product side). That is because the Le Chatelier's Principle states, if the reaction condition of an equilibrium system is changed, the equilibrium position will shift in a way to REDUCE the effect of the change. When the equilibrium position shifts to the left in the above system, that means the forward reaction rate increases (the backward reaction rate remains the same). More product is hence produced, in this case, Fe(SCN)2+(aq).Conversely, if you add Fe(SCN)2+(aq), the equilibrium position shifts to the right (i.e. the reactant side). This time the backward reaction rate increases while the forward reaction rate remains, hence more reactants (Fe3+(aq) and SCN-(aq)) are produced.The concentration effect on equilirium can sometimes be observed. In the above reaction, Fe3+(aq) is yellow, SCN-(aq) is colourless and Fe(SCN)2+(aq)is deep red. If the equilibrium position shifts to the left due to the concentration effect, more Fe(SCN)2+(aq) is produced and the colour of the reaction mixture becomes darker, due to the colour of Fe(SCN)2+(aq). Conversely, if the equilibrium position shifts to the right, the colour becomes paler.
How would the equilibrium concentration of H2O be affected by adding a catalyst to the mixture?
None. A catalyst affects only the rate of reaction, and if the reaction is already at equilibrium, the net rate of the reaction is zero and remains so after a catalyst is added.
What is difference between external and internal indicators used in titration?
Internal indicators that are used in titration exist in the titration reaction as either a reactant or a product. External indicators is added to the reaction mixture, but does not exist in the reaction.
What does it mean if arrows in a chemical reaction are the same length?
Two half arrows are usually used to denote a reaction which is in equilibrium. If they are the same length to one another then equilibrium is obtained and you have a mixture of reagent and product. If the arrow pointing right is larger then this denotes that the reaction is predominently a forwards reaction and favours the product and vice versa.
What is the difference between dissociation constant and equilibrium constant?
Equilibrium constants aren't changed if you change the concentrations of things present in the equilibrium. The only thing that changes an equilibrium constant is a change of temperature. The position of equilibrium is changed if you change the concentration of something present in the mixture. According to Le Chatelier's Principle, the position of equilibrium moves in such a way as to tend to undo the change that you have made.
