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CONSIDER THE FOLLOWING REACTION:
Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq)
A solution is made containing an initial [Fe3+] of
1.2×10−3 M and an initial [SCN−] of
8.2×10−4 M. At equilibrium, [FeSCN2+] =
1.6×10−4 M .
PART A: Calculate the value of the equilibrium constant (Kc): [Express your answer using two significant figures]
KC = _____________________________
The constant Kc is calculated:
Kc = [FeSCN + 2] / [Fe + 3] eq * [SCN-] eq = (1.6x10 ^ -4) / (1.2x10 ^ -3 - 1.6x10 ^ -4) * (8.2x10 ^ -4 - 1.6x10 ^ -4) = 233.1
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* PLEASE WRITE OUT ANSWER STEP BY STEP! CONSIDER THE FOLLOWING REACTION: Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq) A solution is...
Consider the following reaction: Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq) A solution is made containing an initial [Fe3+] of 1.2×10−3 M and an initial [SCN−] of 8.2×10−4 M . At equilibrium, [FeSCN2+]= 1.8×10−4 M . Calculate the value of the equilibrium constant (Kc)(Kc). Express your answer using two significant figures.
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Review |Constants Periodic Table Consider the following reaction: Fe (aq) SCN (aq)FeSCN?+(aq) A solution is made containing an initial | Fe | of 1.2x10-3 M and an initial [SCN of 8.2x104 M At equilibrium, |FeSCN2+-1.8x10-4 M. We were unable to transcribe this image Review |Constants Periodic Table Consider the following reaction: Fe (aq) SCN (aq)FeSCN?+(aq) A solution is made containing an initial | Fe | of 1.2x10-3 M and an initial [SCN of 8.2x104 M At equilibrium, |FeSCN2+-1.8x10-4 M.
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When solutions containing Fe3+(aq) ions and SCN−(aq) ions are mixed together, the following equilibrium is established: Fe3+(aq)+SCN−(aq)⇌FeSCN2+(aq) At equilibrium at some temperature, in 3.0 liters of total solution, there are 0.653 moles of FeSCN2+(aq), 0.0385 moles of Fe3+(aq) and 0.0465 moles of SCN−(aq) . What is K?
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