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For the reversible reaction
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which k values would indicate that there is more B than A at equilibrium?
1, K = 9×10-9
2, K = 0.2
3, K = 9000
4, K = 9×109
♦ Relevant knowledge
The chemical process that is able to proceed simultaneously in both directions is called an irreversible reaction. Being a closed system, it can progress through time from the beginning conditions to reach a point of equilibrium chemical. The concentrations of the aqueous and gaseous reactions in the state of equilibrium can be used to determine the continuous Kc for the reaction temperature. The is always positive. Kc is crucial because its value indicates which side of the reaction favoured in the equilibrium state at the temperature.
This concept is based upon the equilibrium constant of chemical reactions.
The equilibrium constant is the value of the reaction coefficient at equilibrium. It is the ratio between the concentrations in products and reactants.
To perform a chemical reaction
[katex]a{\rm{A}} + b{\rm{B}} \to c{\rm{C}} + d{\rm{D}}[/katex]
As follows is the equation constant.
[katex]K = \frac{{{{\left[ {\rm{C}} \right]}^c}{{\left[ {\rm{D}} \right]}^d}}}{{{{\left[ {\rm{A}} \right]}^a}{{\left[ {\rm{B}} \right]}^b}}}[/katex]
Here [katex]\left[ {\rm{C}} \right][/katex]
The reaction is here
As follows is the equation constant.
[katex]K = \frac{{\left[ {\rm{B}} \right]}}{{\left[ {\rm{A}} \right]}}[/katex]
K, 0.2, and [katex]9 \times {10^{ – 9}}[/katex] are the values.
The values of K, 9000, and [katex]9 \times {10^9}[/katex]Ans are:
K is the value at which A is greater than B. These values are 9000 and [katex]9 \times {10^9}[/katex].