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How will a change in pressure and concentration affect the yield of ammonia made?
Per the Haber process, increasing the pressure moves the equilibrium position to the right, increasing the yield.
Can equilibrium constants be negative?
No. An equilibrium constant is derived from the products, powers, and ratios of the activities (essentially the concentrations) of the species that are in equilibrium. Since there is no such thing as a negative concentration, there is no way their products, powers or ratios can yield a negative number.
How can the magnitude of an equilibrium constant indicate the extent of a reaction?
The reaction proceeds to a very large extent if Kc >> 1. On the other hand, the reaction hardly proceeds if Kc << 1.
How does an increase in pressure affect the following reaction. CO2 plus H2O equals H2CO3?
You get an increased yield of H2CO3, as the equilibrium shifts to the side with fewer moles.
Why does changing the concentration of reactant shift the equilibrium?
Le Chatlier's PrincipleIf an equilibrium reaction is occurring and some reactant from either side of the equilibrium is added, the reaction goes in a direction that is to oppose the addition of a reactant. For example. In the equilibrium of CO2 + H2O = H2CO3, if more CO2 is added then the equilibrium shifts in such a way that this change is opposed so more H2CO3 is produced. For more information, research Le Chatlier's Principle.
What happens to the amount of product when you use a catalyst in equilibrium?
The yield of reaction is improved.
How will a change in pressure and concentration affect the yield of ammonia made?
Per the Haber process, increasing the pressure moves the equilibrium position to the right, increasing the yield.
Can equilibrium constants be negative?
No. An equilibrium constant is derived from the products, powers, and ratios of the activities (essentially the concentrations) of the species that are in equilibrium. Since there is no such thing as a negative concentration, there is no way their products, powers or ratios can yield a negative number.
Why a reaction needs to take place at equilibrium?
Many chemical reactions, like combustion , go to completion and not to equilibrium. It is normally desirable to give a chemical reaction time to reach equilibrium in order you get the maximum yield of one or more products.
How can the magnitude of an equilibrium constant indicate the extent of a reaction?
The reaction proceeds to a very large extent if Kc >> 1. On the other hand, the reaction hardly proceeds if Kc << 1.
How would the yield of ethanol at equilibrium change if the temperature was increased?
If you raise the temperature, the endothermic reaction will increase to use up the extra heat, therefore producing less percentage yield of ethanol and more of ethene and steam.
How does an increase in pressure affect the following reaction. CO2 plus H2O equals H2CO3?
You get an increased yield of H2CO3, as the equilibrium shifts to the side with fewer moles.
In a reverse reactionproducts are formed from reactants and reactants are formed from products When they yield the same amount?
Of material. They will need to have the same amount of atoms present for this process to work out correctly.
Why does changing the concentration of reactant shift the equilibrium?
Le Chatlier's PrincipleIf an equilibrium reaction is occurring and some reactant from either side of the equilibrium is added, the reaction goes in a direction that is to oppose the addition of a reactant. For example. In the equilibrium of CO2 + H2O = H2CO3, if more CO2 is added then the equilibrium shifts in such a way that this change is opposed so more H2CO3 is produced. For more information, research Le Chatlier's Principle.
Reactants are CO2 and H2O?
Carbon dioxide (CO2) and (H20) are the reactants that yield the product of carbonic acid (H2C03). The reaction occurs in both (equilibrium) directions by the formula H20 + CO2 <-->H2CO3.
To maximize equilibrium yield of methanol would you use high or low temperature?
High because a higher pressure is the result of decreased volume and when a decreased volume for the equilibrium mixture is involved, the shift is toward the side with the least amount of mols of gas. 3 for reactants and 1 for methanol so towards methanol
What effect does increasing pressure have on the yield of ammonia in the Haber process?
It increases the yield. 3 moles of hydrogen react with one mole of nitrogen to produce two moles of ammonia. As there is a REDUCTION in molecules, there will be a reduction in pressure. This is alsos an equilibrium reaction. So by Le Chetalier's principle, if we increase pressure, the system will react to reduce the pressure again. This can be done by producing more ammonia - in other words, an increase in product yield.
