Electrochemistry

The reaction taking place in a galvanic cell is as given

\(\mathrm{A}(\mathrm{s})+\mathrm{B}^{2+}\left(\mathbf{1} \mathbf{1} \mathbf{1 0} \mathbf{0}^{-\mathrm{M}} \mathbf{M}\right) \rightarrow \mathrm{B}_{(\mathrm{s})}+\mathrm{A}^{2+}(0.1 \mathrm{M}).\)

The emf of the cell is \(+2.651 \mathrm{~V}\). If the standard emf of the cell is \(+2.71 \mathrm{~V}\), what is the value of \(\mathrm{X}\) ?