Question
Answer the following questions:
Write balanced equations to represent what happens when.
  1. Cu2+ is treated with KI.
  2. Acidified potassium dichromate solution is reacted with iron (II) solution. (ionic equation).

Answer

  1. $2\text{Cu}^{2+}4\text{I}^-\xrightarrow{\ \ \ \ \ \ \ \ }2\text{Cr}^{3+}+7\text{H}_2\text{O}$

$\text{Cr}_2\text{O}^{2-}_7+14\text{H}^++6\text{e}^-\xrightarrow{ \ \ \ \ \ \ \ \ }2\text{Cr}^{3+}+7\text{H}_2\text{O}$

  1. $\text{Fe}^{2+}\xrightarrow{\ \ \ \ \ \ \ \ \ }\text{Fe}^{3+}+\text{e}^-]\times6$

$\text{Cr}_2\text{O}^{2-}_+6\text{Fe}^{2+}+14\text{H}^+\xrightarrow{\ \ \ \ \ \ \ \ \ }2\text{Cr}^{3+}+6\text{Fe}^{3+}+7\text{H}_2+\text{O}$

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Similar questions

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Column I (Coordination Compound)
 
Column II (Central metal atom)
a.
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1.
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b.
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c.
Wilkinson catalyst
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4.
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5.
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Code:
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  2. A (3), B (4), C (5), D (1).
  3. A (4), B (3), C (2), D (1).
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(iii) For a first order reaction, if the rate constant at 500 K and 600 K are $0.03 s^{-1}$ and $0.06 s^{-1}$ respectively, then calculate the activation energy.
$
\left[R=8.314 JK^{-1} mol^{-1}, \log 2=0.3010\right]
$
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