The standard electromotive force (EMF) of an electrochemical cell is determined by the difference between the standard electrode potentials of the cathode and anode, as expressed by the equation:\[\text{EMF} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}}\]In this formula:- \( E^\circ_{\text{cathode}} \) denotes the standard reduction potential at the cathode, where reduction occurs.- \( E^\circ_{\text{anode}} \) denotes the standard reduction potential at the anode, where oxidation occurs.The provided standard electrode potentials are:- For \( \text{Zn}^{2+}/\text{Zn} \): \( -0.76 \, \text{V} \)- For \( \text{Cu}^{2+}/\text{Cu} \): \( +0.34 \, \text{V} \).In a galvanic cell, the half-cell with the higher standard reduction potential functions as the cathode (site of reduction), while the half-cell with the lower standard reduction potential acts as the anode (site of oxidation). Comparing the given potentials:- \( E^\circ (\text{Cu}^{2+}/\text{Cu}) = +0.34 \, \text{V} \) is the higher potential, thus designated as the cathode.- \( E^\circ (\text{Zn}^{2+}/\text{Zn}) = -0.76 \, \text{V} \) is the lower potential, thus designated as the anode.The cell representation is:\[\text{Zn} | \text{Zn}^{2+} || \text{Cu}^{2+} | \text{Cu}\]The standard EMF is calculated as:\[\text{EMF} = E^\circ_{\text{Cu}^{2+}/\text{Cu}} - E^\circ_{\text{Zn}^{2+}/\text{Zn}}\]Substituting the values:\[\text{EMF} = 0.34 \, \text{V} - (-0.76 \, \text{V}) = 0.34 \, \text{V} + 0.76 \, \text{V} = 1.10 \, \text{V}\]A positive EMF value signifies that the cell reaction proceeds spontaneously as depicted.Therefore, the standard EMF of the described cell is \( 1.10 \, \text{V} \).