Question

When the $Ag^+$ concentration is $8.60 \times 10^{-4}$ M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 1.796V. What is the $Mn^{2+}$ concentration? $2Ag^+(aq) + Mn(s) \rightarrow 2Ag(s) + Mn^{2+}(aq)$ $[Mn^{2+}] = \text{______} M$

Name: when the ag concentration is 860 times 10 4 m the observed cell potential at 298 k for an electrochemical cell with the following reaction is 1796v what is the mn2 concentration 2agaq mns ri 16603
Uploaded: 2023-05-22T08:58:24-08:00
Duration: 1 min 47 s
Channel: Madhur L
Description: when the ag concentration is 860 times 10 4 m the observed cell potential at 298 k for an electrochemical cell with the following reaction is 1796v what is the mn2 concentration 2agaq mns ri 16603

          When the $Ag^+$ concentration is $8.60 \times 10^{-4}$ M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 1.796V. What is the $Mn^{2+}$ concentration?
$2Ag^+(aq) + Mn(s) \rightarrow 2Ag(s) + Mn^{2+}(aq)$
$[Mn^{2+}] = \text{______} M$

when the ag concentration is 860 times 10 4 m the observed cell potential at 298 k for an electrochemical cell with the following reaction is 1796v what is the mn2 concentration 2agaq mns ri 16603

Added by Lisa M.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Madhur L

05/22/2023

Step 1

314 J/mol·K) T is the temperature in Kelvin (298 K) n is the number of electrons transferred (2 in this case) F is the Faraday constant (96485 C/mol) Q is the reaction quotient Show more…

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When the $Ag^+$ concentration is $8.60 \times 10^{-4}$ M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 1.796V. What is the $Mn^{2+}$ concentration? $2Ag^+(aq) + Mn(s) \rightarrow 2Ag(s) + Mn^{2+}(aq)$ $[Mn^{2+}] = \text{______} M$