We appreciate your visit to Enter your answer in the provided box The equilibrium constant for the reaction Sr s Mg 2 aq Sr 2 aq Mg s is 2. This page offers clear insights and highlights the essential aspects of the topic. Our goal is to provide a helpful and engaging learning experience. Explore the content and find the answers you need!
Answer :
Final answer:
The standard cell potential (E0) for a cell made up of Sr/Sr2+ and Mg/Mg2+ half-cells at 25 degrees Celsius, given an equilibrium constant of 2.69×10^12, can be calculated to be 0.88V.
Explanation:
We can calculate the standard cell potential, E0, using the equation derived from the Nernst Equation: E0 = 0.0592/n * log(K) (at 25 degrees Celsius), where n is the number of electrons transferred in the balanced redox reaction, and K is the equilibrium constant.
In our case, the equilibrium constant (K) is given as 2.69×10^12. The balanced equation shows that n=2. Plugging these values into the formula, we get: E0 = 0.0592/2 * log(2.69×10^12). Calculating this gives us E0 = 0.88V.
Therefore, the standard cell potential for a cell made up of Sr/Sr2+ and Mg/Mg2+ half-cells at 25 degrees Celsius is 0.88V.
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Thanks for taking the time to read Enter your answer in the provided box The equilibrium constant for the reaction Sr s Mg 2 aq Sr 2 aq Mg s is 2. We hope the insights shared have been valuable and enhanced your understanding of the topic. Don�t hesitate to browse our website for more informative and engaging content!
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In this question, we are asked to calculate the standard cell potential of a reaction given the equilibrium constant. Using the Nernst equation, we can relate the standard cell potential to the equilibrium constant. By rearranging the Nernst equation and plugging in the given values, we can calculate the standard cell potential.
The equilibrium constant, Kc, can be related to the standard cell potential, E0, using the Nernst equation: E = E0 - (RT/nF) ln(Kc). In this case, the reaction is Sr(s) + Mg2+(aq) ⇌ Sr2+(aq) + Mg(s). Since the reaction is at equilibrium, the cell potential is zero, so E0 can be calculated by rearranging the Nernst equation: E0 = (RT/nF) ln(Kc). R is the ideal gas constant, T is the temperature in Kelvin, n is the number of electrons transferred, and F is Faraday's constant.
Given Kc = 2.69×1012 and assuming the temperature is 25°C, we can convert it to Kelvin (298 K) and calculate E0. Since no information is provided regarding the number of electrons transferred, we assume it is two (as the equation suggests).
Using the appropriate values, we can plug them into the equation to calculate E0. After determining E0, it can be converted to volts (V) by dividing by 1000.
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