Cell Potential and Free Energy Practice Test

A galvanic cell is assembled under standard conditions with the anode labeled as an Al(s)|Al$^{3+}$(aq) electrode and the cathode labeled as a Ag$^+$(aq)|Ag(s) electrode. A student claims the overall cell reaction is spontaneous. Which statement correctly describes the sign of $E^\circ_{\text{cell}}$ and spontaneity for the cell as labeled?

A student builds a cell under standard conditions using a Sn(s)|Sn$^{2+}$(aq) half-cell and a Ag(s)|Ag$^+$(aq) half-cell. The standard reduction potentials are: Sn$^{2+}$ + 2e$^-$ $\rightarrow$ Sn(s), $E^\circ = -0.14,\text{V}$; Ag$^+$ + e$^-$ $\rightarrow$ Ag(s), $E^\circ = +0.80,\text{V}$. The student writes the overall reaction as Sn$^{2+}$(aq) + 2Ag(s) $\rightarrow$ Sn(s) + 2Ag$^+$(aq). Which statement is correct about this written reaction under standard conditions?