does the voltaic cell(in exp) must be the same with the standard cell that we calculated based on the formula?
In an electrochemical experiment, a voltaic cell is created by combining two half-cells. Each half-cell consists of an electrode immersed in an electrolyte solution. The overall cell potential of a voltaic cell is determined by the reaction that occurs at the electrode-electrolyte interface in each half-cell.
The standard cell potential, also known as the standard electrode potential, is the potential difference between two half-cells under specific standard conditions. It is usually represented by E°. The standard cell potential allows us to predict whether a redox reaction is spontaneous or non-spontaneous.
Now, to answer your question: No, the voltaic cell in an experiment doesn't necessarily have to be the same as the standard cell calculated based on a balanced equation. In experiments, it is common to have deviations from ideal conditions due to various factors like concentration changes, temperature differences, or impurities in the electrolyte.
However, it is important to note that the standard cell potential is still useful in experiments because it provides a reference point for comparing the observed cell potential with the calculated standard cell potential. The difference between the observed and standard cell potentials, called the cell potential deviation, can provide valuable insights into the experimental conditions and the behavior of the electrochemical system.
In summary, while the voltaic cell in an experiment might not perfectly match the standard cell calculated based on the balanced equation, the standard cell potential remains a crucial parameter for understanding the electrochemical process and evaluating experimental results.