If the same materials are used to build a voltaic cell and an electrolytic cell, how would the chemical reactions compare?
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The same overall reaction would happen in each cell, but it would take place spontaneously in the voltaic cell.
The same overall reaction would happen in each cell, but it would take place nonspontaneously in the voltaic cell.
The reaction in the voltaic cell would be nonspontaneous and the reverse of the reaction in the electrolytic cell.
The reaction in the voltaic cell would be spontaneous and the reverse of the reaction in the electrolytic cell.

Hno3(aq) → h+(aq) + no3−(aq). picture ii best represents the strong acid hno3. strong acids are strong electrolytes

Idon't know hope someone you

Answerthis solution will not form a precipitateexplanationsolubility equilbrium:         pbf₂(s)  ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is    (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as    then, we can interpret  q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually  forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product:     since q = 2.7  × 10⁻⁸ < ksp =  4  ×  10⁻⁸, a precipitate will not form.