MCQ
Which is not a colligative property
- ✓Refractive index
- BLowering of vapour pressure
- CDepression of freezing point
- DElevation of boiling point
✓
Answer
Correct option: A.
Refractive index
a
Colligative properties depend on how many solute particles are present as well as the solvent amount, but they do NOT depend on the type of solute particles.
Colligative properties depend on how many solute particles are present as well as the solvent amount, but they do NOT depend on the type of solute particles.
Hence, Refractive Index is not a colligative particles as it only depends on nature of materials.
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Use the data and find out the most stable oxidised species.
$\text{E}^\ominus_{\text{cr}_2\text{O}^{2-}_7/\text{cr}^{3+}}=1.33\text{V}\ \ \ \text{E}^\ominus_{\text{Cl}_2/\text{Cl}^-}=1.36\text{V}$
$\text{E}^\ominus_{\text{MnO}^-_4/\text{Mn}^{2+}}=1.51\text{V}\ \ \ \ \text{E}^\ominus_{\text{Cr}^{3+}/\text{Cr}}=-0.74\text{V}$
→$\text{E}^\ominus_{\text{cr}_2\text{O}^{2-}_7/\text{cr}^{3+}}=1.33\text{V}\ \ \ \text{E}^\ominus_{\text{Cl}_2/\text{Cl}^-}=1.36\text{V}$
$\text{E}^\ominus_{\text{MnO}^-_4/\text{Mn}^{2+}}=1.51\text{V}\ \ \ \ \text{E}^\ominus_{\text{Cr}^{3+}/\text{Cr}}=-0.74\text{V}$
Redox reactions play a pivotal role in chemistry and biology. The values of standard redox potential ( $\mathrm{E}^{\circ}$ ) of two half-cell reactions decide which way the reaction is expected to proceed. A simple example is a Daniel cell in which zinc goes into solution and copper gets deposited. Given below are a set of half-cell reactions (acidic medium) along with their $E^{\circ}$ ($V$ with respect to normal hydrogen electrode) values.
→$\mathrm{I}_2+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{I}\ \ \ \mathrm{E}^{\circ}=0.54 $
$\mathrm{Cl}_2+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cl}^{-} \ \ \ \mathrm{E}^{\circ}=1.36 $
$\mathrm{Mn}^{3+}+\mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+} \ \ \ \mathrm{E}^{\circ}=1.50 $
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$\mathrm{O}_2+4 \mathrm{H}^{+}+4 \mathrm{e}^{-} \rightarrow 2 \mathrm{H}_2 \mathrm{O} \ \ \ \mathrm{E}^{\circ}=1.23$
$1.$ Among the following, identify the correct statement.
$(A)$ Chloride ion is oxidized by $\mathrm{O}_2$
$(B)$ $\mathrm{Fe}^{2+}$ is oxidized by iodine
$(C)$ Iodide ion is oxidized by chlorine
$(D)$ $\mathrm{Mn}^{2+}$ is oxidized by chlorine
$2.$ While $\mathrm{Fe}^{3+}$ is stable, $\mathrm{Mn}^{3+}$ is not stable in acid solution because
$(A)$ $\mathrm{O}_2$ oxidises $\mathrm{Mn}^{2+}$ to $\mathrm{Mn}^{3+}$
$(B)$ $\mathrm{O}_2$ oxidises both $\mathrm{Mn}^{2+}$ and $\mathrm{Fe}^{2+}$ to $\mathrm{Fe}^{3+}$
$(C)$ $\mathrm{Fe}^{3+}$ oxidizes $\mathrm{H}_2 \mathrm{O}$ to $\mathrm{O}_2$
$(D)$ $\mathrm{Mn}^{3+}$ oxidises $\mathrm{H}_2 \mathrm{O}$ to $\mathrm{O}_2$
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$(C)$ $\mathrm{Fe}_4\left[\mathrm{Fe}(\mathrm{CN})_6\right]_2$ $(D)$ $\mathrm{Fe}_3\left[\mathrm{Fe}(\mathrm{CN})_6\right]_3$
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