Cell Potential Under Nonstandard Conditions Practice Test

A galvanic cell operates using the half-cells $\text{Cd}(s)|\text{Cd}^{2+}(aq)$ and $\text{Ag}^+(aq)|\text{Ag}(s)$. The spontaneous overall reaction under standard conditions is $$\text{Cd}(s)+2\text{Ag}^+(aq)\rightarrow \text{Cd}^{2+}(aq)+2\text{Ag}(s).$$ Compared with standard conditions, the $\text{Ag}^+$ concentration is increased above $1.0,\text{M}$ while all other species remain at standard conditions. Using qualitative Nernst reasoning (by comparing $Q$ to its standard-condition value), what happens to $E_\text{cell}$ and spontaneity?

A galvanic cell is constructed at $25^\circ\text{C}$ using the half-cells $\text{Zn}(s)|\text{Zn}^{2+}(aq)$ and $\text{Cu}^{2+}(aq)|\text{Cu}(s)$, connected by a salt bridge. Compared with standard conditions, the $\text{Zn}^{2+}$ concentration is increased above $1.0,\text{M}$ while all other species remain at standard conditions. Using qualitative Nernst reasoning (by determining how $Q$ changes relative to standard conditions), how does the cell potential $E_\text{cell}$ change and does the cell remain spontaneous?