For a reacton, aA <-----> bB, you start with 5 mole of reactant A and 0 mol of r

Question

For a reacton, aA <-----> bB, you start with 5 mole of reactant A and 0 mol of reactant B in a 1.0L flask.

a. explain what happens to the rate at which A --> B over time. Explain why this occurs.

b. explain what happens to the rate at which B --> A over time. Explain why this occurs.

c. expalin how equilibrium is achieved and identify exactly what it means.

d. if B-->A did not occur, only A-->B did, would you reach an equilibrium state where some product and some reactants would reamin ropesnent in the reaction container? Explain.

Explanation / Answer

a) A --------> B

At the beginning concentration of reactant is higher, so, reactant A is consumed , the same amount of product B would be formed,then the rate of forward reaction increases.

b) B ---------> A

Because of forward reaction, concentration of B is increased. Once concentration of B is increased, backward reaction takes place. Then the rate of backward reaction increases, and rate of forward reaction decreases.

c) Because of the above two reactions, at a time, the rate of forward reaction and rate of backward reaction will become equal and that state is called equillibrium state.

At equllibrium, rate of forward reaction = rate of backward reaction

d) if B-->A did not occur, only A-->B did, equilibrium would not be reached.

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