We are being asked to determine which will give a greater partial pressure at equilibrium for the given reaction
A(g) ⇌ B(g)
We are given the two elementary processes and their rate constant.
A→B ; k = 4.7 x 10-3 s-1
B → A ; k = 5.8 x 10-1 s-1
Recall: Associated with any reaction at equilibrium is the equilibrium constant K.
Its numerical value determines if reactants or products are more greatly favored within a reaction.
If K > 1 then the products > reactants and the forward direction is favored.
If K < 1 then the products < reactants and the reverse direction is favored.
If K = 1 then the products = reactants.
The equilibrium constant, K, can be expressed as the ratio of the forward and reverse rate constant
Suppose that the gas-phase reactions A → B and B→ A are both elementary processes with rate constants of 4.7 x 10-3 s-1 and 5.8 x 10-1 s-1, respectively.
Which is greater at equilibrium, the partial pressure of A or the partial pressure of B?
A(g) ⇌ B(g)
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