When does chemical equilibrium result?
When the forward rate is equivalent to the reverse rate of reaction.
By definition, chemical equilibrium occurs when the forward rate is equivalent to the reverse rate:
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Chemical equilibrium results when the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products remain constant over time.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
- How do we formulate #"iodide ion"# in aqueous solution?
- In the reaction between #HNO_2# and #HCN#: #HNO_2(aq) + CN^(-)(aq) rightleftharpoons HCN(aq) + NO_2^(-)(aq)#, K = #1 x 10^6#. What are the predominate species after the reaction reaches equilibrium?
- How do you calculate the Keq of a reaction?
- A chemical reaction always tries to go to completion, one way or the other If there is a way for the reaction to go the reverse direction, what is this process called?
- Consider this chemical reaction: #H_2(g) + I_2(g) rightleftharpoons 2HI(g)#. At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were 0.15 M, 0.033 M, and 0.55 M, respectively. What is the value of #K_(eq)# for this reaction?

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