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PART - 1 CH - 6 Equilibrium — Chemistry STD 11 Science — Question

Gujarat BoardEnglish MediumSTD 11 ScienceChemistryPART - 1 CH - 6 Equilibrium5 Marks
Question
Explain with examples the terms necessary to determine the pH of weak electrolyte solution.
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The value of $K _{ p }$ for the reaction,
$
CO_2(g)+C(s) \rightleftharpoons 2 CO(g)
$
is 3.0 at 1000 K . If initially, $P_{ CO _2}=0.48$ bar and $P _{ CO }=0$ bar and pure graphite is present, calculate the equilibrium partial pressures of CO and $CO _2$.
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Nitric oxide reacts with $Br_2$ and gives nitrosyl bromide as per reaction given below:
$2\text{NO (g) + Br}_2\text{ (g)}\leftrightharpoons2\text{NOBr (g)}$
When $0.087$ mol of $NO$ and $0.0437$ mol of $Br _2$ are mixed in a closed container at constant temperature, $0.0518$ mol of $NOBr$ is obtained at equilibrium. Calculate equilibrium amount of $NO$ and $Br _2$.
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Calculate (a) $\Delta \text{G}^\ominus$ (b) the equilibrium constant for the formation of $NO_2$ from NO and $O_2$​​​​​​​ at 298K
$\text{NO (g) + }1/2\text{ O}_2\text{ (g)}\rightleftharpoons\text{NO}_2\text{ (g)}$
where
$\Delta_\text{r}\text{G}^\ominus\text{ (NO}_2)=52.0\text{ kJ/mol}$
$\Delta_\text{r}\text{G}^\ominus\text{ (NO})=87.0\text{ kJ/mol}$
$\Delta_\text{r}\text{G}^\ominus\text{ (O}_2)=0\text{ kJ/mol}$
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Match the species in Column I with the type of hybrid orbitals in Column II.
 
Column I
 
Column II
i.
$SF_4$
a.
$sp^3d^2$
ii.
$IF_5$
b.
$d^2sp$
iii.
 $\text{NO}^{+}_{2}$
c.
$sp^3d$
iv.
 $\text{NH}^{+}_{4}$
d.
$sp^3$
 
  
e.
 $Sp$
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 The solubility product of AgCl is $1.5 \times 10^{-10}$. Predict whether there will be any precipitation by mixing $50 mL$ of $0.01 M NaCl$ and $50 mL$ of $0.01 M AgNO _3$ solution.
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Consider the cell reaction of an electrochemical cell:
$\text{Ni}\text{(s)}+2\text{Ag}^+\text{(aq)}\xrightarrow{\ \\ \ \ \ \ }\text{Ni}^{2+}\text{(aq)}+2\text{Ag}\text{(s)}$
Answer the following questions:
  1. Write anode and cathode half reactions.
  2. Mention the direction of flow of electrons.
  3. How is the electroneutrality maintained in solution of two half cells?
  4. Write the formula for calculating standard e.m.f of this cell.
  5. How does e.m.f. change when concentration of $Ag^+$ is decreased?
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Explain the reason for the fusion of an organic compound with metallic sodium for testing nitrogen, sulphur and halogens.
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The concentration of sulphide ion in $0.1$ M HCl solution saturated with hydrogen sulphide is $1.0 \times 10^{-19} \mathrm{M}$. If $10$ mL of this is added to $5$ mL of $0.04$ M solution of the following: $\mathrm{FeSO}_4, \mathrm{MnCl}_2, \mathrm{ZnCl}_2$ and $\mathrm{CdCl}_2$. in which of these solutions precipitation will take place?
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Write the expression for the equilibrium constant, $K _{ C }$ for each of the following reactions:
a. $2 NOCl ( g ) \rightleftharpoons 2 NO ( g )+ Cl _2(g)$
b. $2 Cu \left( NO _3\right)_2(s) \rightleftharpoons 2 CuO ( s )+4 NO _2(g)+ O _2(g)$
c. $CH _3 COOC _2 H _5( aq )+ H _2 O ( l ) \rightleftharpoons CH _3 COOH ( aq )+ C _2 H _5 OH ( aq )$
d. $Fe ^{3+}( aq )+3 OH ^{-}( aq ) \rightleftharpoons Fe ( OH )_3(s)$
e. $I _2(s)+5 F_2 \rightleftharpoons 2 IF _5$
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Explain the important aspects of resonance with reference to the $\text{CO}^{2-}_3$− ion.
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