Determine the direction of spontaneity of the following pairs of substances: a. Sn with Cd+2 b. Cd+2 with H+ c. Cd with H2 d. Cd with Sn+2
Understand the Problem
The question asks us to determine the spontaneity of reactions between pairs of substances. This involves considering the standard reduction potentials of the substances involved and using them to predict whether a redox reaction will occur spontaneously. The more positive the reduction potential, the greater the tendency for the species to be reduced. A spontaneous reaction will occur if the reduction half-reaction has a higher reduction potential than the oxidation half-reaction.
Answer
Compare standard reduction potentials (E°) for each pair; a positive overall cell potential (E°cell) indicates a spontaneous reaction. Accessing a table of standard reduction potentials is necessary to determine the specific spontaneity for each reaction.
To determine spontaneity, compare the standard reduction potentials (E°) of each half-reaction. A reaction is spontaneous if the overall cell potential (E°cell) is positive. This occurs when a stronger oxidizing agent reacts with a stronger reducing agent. You'll need a table of standard reduction potentials to compare the E° values for each substance. Unfortunately, I don't have access to a specific table of values to provide a definitive answer.
Answer for screen readers
To determine spontaneity, compare the standard reduction potentials (E°) of each half-reaction. A reaction is spontaneous if the overall cell potential (E°cell) is positive. This occurs when a stronger oxidizing agent reacts with a stronger reducing agent. You'll need a table of standard reduction potentials to compare the E° values for each substance. Unfortunately, I don't have access to a specific table of values to provide a definitive answer.
More Information
The standard reduction potential is a measure of the tendency of a chemical species to be reduced. The more positive the reduction potential, the greater the species' affinity for electrons and tendency to be reduced. The standard cell potential (E°cell) for an electrochemical cell is determined by the difference between the reduction potentials at the cathode (reduction) and anode (oxidation): E°cell = E°(cathode) - E°(anode).
Tips
A common mistake is to forget to reverse the sign of the standard reduction potential when the half-reaction is written as an oxidation.
Sources
- Comparing Strengths of Oxidants and Reductants - chem.libretexts.org
- Spontaneity of Redox Reactions - kcourses.weebly.com
- Predict whether the following reactions would occur spontaneously ... - vaia.com
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