Question
Explain relationship between $E _{\text {cell }}^{\circ}$ and equilibrium constant with the help of Nernst equation.

Answer

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Answer the following question:
$0.6\ mL$ of acetic acid $(CH_3COOH),$ having density $1.06\ g\ mL^{-1},$ is dissolved in $1$ litre of water. The depression in freezing point observed for this strength of acid was $0.0205^\circ C.$ Calculate the van’t Hoff factor and the dissociation constant of acid.
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Write the applications of d- and f-block elements.
Differentiate between DNA and RNA.
Write the principle of manufacture of ammonia by Haber's process. How does it react with $ CuSO_{4} $ solution?
Vapour pressures of pure acetone and chloroform at 328 K are 741.8 mm Hg and 632.8 mm Hg respectively. Assuming that they form ideal solution over the entire range of composition, plot $p_{\text {total }}, p_{\text {chloroform }}$ and $p_{\text {acetone }}$ as a function of $x_{\text {acetone }}$ The experimental data observed for different compositions of mixture is :
$100 \times x_{\text {acetone }}$011.823.436.050.858.264.572.1
$p_{\text {acetone }} / mm Hg$054.9110.1202.4322.7405.9454.1521.1
$p_{\text {chloroform }} / mm Hg$632.8548.1469.4359.7257.7193.6161.2120.7
Plot this data also on the same graph paper. Indicate whether it has positive deviation or negative deviation from the ideal solution.
Draw the structures of optical isomers of:
i. $\left[ Cr \left( C _2 O _4\right)_3\right]^{3-}$
ii. $\left[ PtCl _2( en )_2\right]^{2+}$
iii. $\left[ Cr \left( NH _3\right)_2 Cl _2( en )\right]^{+}$