Chemistry Question from JEE Main 2023 · 6 April, Shift 1

The standard reduction potentials at $298 \, \text{K}$ for the following half cells are given below:

$\text{NO}_3^- + 4\text{H}^+ + 3e^- \rightarrow \text{NO(g)} + 2\text{H}_2\text{O}, \; E^0 = 0.97 \, \text{V}$ $\text{V}^{2+}\text{(aq)} + 2e^- \rightarrow \text{V}, \; E^0 = -1.19 \, \text{V}$ $\text{Fe}^{3+}\text{(aq)} + 3e^- \rightarrow \text{Fe}, \; E^0 = -0.04 \, \text{V}$ $\text{Ag}^+\text{(aq)} + e^- \rightarrow \text{Ag(s)}, \; E^0 = 0.80 \, \text{V}$ $\text{Au}^{3+}\text{(aq)} + 3e^- \rightarrow \text{Au(s)}, \; E^0 = 1.40 \, \text{V}$

The number of metal(s) which will be oxidized by $\text{NO}_3^-$ in aqueous solution is: