At 298K, the EMF of the cell: Mg(s) |Mg2+(Q)||Ag+(0.01)|Ag(s)is 3.022V. Calculate the value ‘Q’.(Given: EoMg2+/Mg = -2.37V and EoAg+/Ag = 0.80V)
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Solution 1
To solve this problem, we need to use the Nernst equation which is:
E = E° - (RT/nF) * lnQ
Where: E is the cell potential, E° is the standard cell potential, R is the gas constant (8.314 J/(mol·K)), T is the temperature in Kelvin, n is the number of moles of electrons transferred in the balanced r Knowee AI StudyGPT is a powerful AI-powered study tool designed to help you to solve study prob
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Knowee AI StudyGPT is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI StudyGPT is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI StudyGPT is a powerful AI-powered study tool designed to help you to solv
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At 298K, the EMF of the cell: Mg(s) |Mg2+(Q)||Ag+(0.01)|Ag(s)is 3.022V. Calculate the value ‘Q’.(Given: EoMg2+/Mg = -2.37V and EoAg+/Ag = 0.80V)
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