Determine whether the following reaction will occur by determining the voltage produced; Ag(s) + HCl(aq) =
Ag(s) + 2HCl(aq) == > AgCl(s) + H2(g)
You will need to look up the Eo value for Ag(s) ==> Ag^+ + 1e.
Look up the Eo value for H^+ +e ==> H2(g)
Add them together. If Erxn is + the reaction will occur as I've written it.
If Erxn is - the reaction will not occur as I've written it.
Post your work if you get stuck.
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To determine whether the given reaction will occur and to find the voltage produced, we need to compare the standard reduction potentials of the species involved.
The half-reactions for the given reaction are:
Ag(s) → Ag+(aq) + e- (Reduction half-reaction)
H2(g) → 2H+(aq) + 2e- (Oxidation half-reaction - from HCl)
The standard reduction potentials for these half-reactions are:
Ag+(aq) + e- → Ag(s) E° = +0.800 V
2H+(aq) + 2e- → H2(g) E° = 0.000 V (reference)
To calculate the overall cell potential, we subtract the reduction potential of the oxidation half-reaction from the reduction potential of the reduction half-reaction:
E° cell = E° reduction - E° oxidation
E° cell = (+0.800 V) - (0.000 V)
E° cell = +0.800 V
The positive value for E° cell indicates that the reaction is spontaneous and will occur. Additionally, the voltage produced by the reaction will be 0.800 V.
To determine whether the reaction between Ag(s) and HCl(aq) will occur, we can look at the redox potentials of the two half-reactions involved and calculate the overall cell potential.
First, let's write the balanced half-reactions for the oxidation and reduction processes:
The oxidation half-reaction: Ag(s) → Ag+(aq) + e-
The reduction half-reaction: 2H+(aq) + 2e- → H2(g)
Next, we need to find the redox potentials (standard reduction potentials) for each half-reaction. These values can be found in reference tables or online.
The standard reduction potential for Ag+ (aq) to Ag(s) is +0.80 V.
The standard reduction potential for 2H+ (aq) to H2(g) is 0.00 V.
To calculate the overall cell potential, we need to subtract the reduction potential of the oxidation half-reaction from the reduction potential of the reduction half-reaction:
Ecell = Ered - Eox
Ecell = 0.00 V - (+0.80 V)
Ecell = -0.80 V
The negative sign indicates that the reaction is not spontaneous under standard conditions. Therefore, the reaction between Ag(s) and HCl(aq) will not occur spontaneously.
Note: The standard potentials used are at standard conditions (1M concentration, 298K temperature). Actual conditions may vary.