The free energy change for the following reaction at 25 °C, when [Fe²+] = 1.18 M and [Cr³+] = 8.62×10-3 M, is -186 kJ: 3FE2*(1.18 M) + 2Cr(s)→3F€(s) + 2Cr**(8.62×10-3 M) AG= -186 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?

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The free energy change for the following reaction at 25 °C, when \([Fe^{2+}] = 1.18 \, \text{M}\) and \([Cr^{3+}] = 8.62 \times 10^{-3} \, \text{M}\), is \(-186 \, \text{kJ}\):

\[ 
3Fe^{2+}(1.18 \, \text{M}) + 2Cr(s) \rightarrow 3Fe(s) + 2Cr^{3+}(8.62 \times 10^{-3} \, \text{M}) \quad \Delta G = -186 \, \text{kJ} 
\]

What is the cell potential for the reaction as written under these conditions?

**Answer:** \_\_\_\_\_ V

Would this reaction be spontaneous in the forward or the reverse direction? \(\bigtriangledown\)
Transcribed Image Text:The free energy change for the following reaction at 25 °C, when \([Fe^{2+}] = 1.18 \, \text{M}\) and \([Cr^{3+}] = 8.62 \times 10^{-3} \, \text{M}\), is \(-186 \, \text{kJ}\): \[ 3Fe^{2+}(1.18 \, \text{M}) + 2Cr(s) \rightarrow 3Fe(s) + 2Cr^{3+}(8.62 \times 10^{-3} \, \text{M}) \quad \Delta G = -186 \, \text{kJ} \] What is the cell potential for the reaction as written under these conditions? **Answer:** \_\_\_\_\_ V Would this reaction be spontaneous in the forward or the reverse direction? \(\bigtriangledown\)
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