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

$\overline{){\mathbf{K}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\frac{\mathbf{products}}{\mathbf{reactants}}{\mathbf{=}}\frac{\mathbf{forward}\mathbf{}\mathbf{rate}}{\mathbf{reverse}\mathbf{}\mathbf{rate}}}$

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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