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Q14 In the equilibrium\[\mathrm{PCl}_{5}(\mathrm{~g}) \square \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \Delta \mathrm{H}=+90 \mathrm{~kJ} \mathrm{~mol}^{-1}\]What is the effect on(a) the position of equilibrium(b) equilibrium constant? ifi) temperature is increased
Q14 In the equilibrium\[\mathrm{PCl}_{5}(\mathrm{~g}) \square  \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g})  \Delta \mathrm{H}=+90 \mathrm{~kJ} \mathrm{~mol}^{-1}\]What is the effect on(a) the position of equilibrium(b) equilibrium constant? ifi) temperature is increased

Q14 In the equilibrium\[\mathrm{PCl}_{5}(\mathrm{~g}) \square \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \Delta \mathrm{H}=+90 \mathrm{~kJ} \mathrm{~mol}^{-1}\]What is the effect on(a) the position of equilibrium(b) equilibrium constant? ifi) temperature is increased

Q8 (a) Write down \mathrm{K}_{c} for the following reversible reactions. Suppose that the volume of reaction mixture in all the cases is V^{\prime \prime} \mathrm{dm}^{3} at equilibrium stage.V) \mathrm{N}_{2}+3 \mathrm{H}_{2} \square 2 \mathrm{NH}_{3}
Q8 (a) Write down  \mathrm{K}_{c}  for the following reversible reactions. Suppose that the volume of reaction mixture in all the cases is  V^{\prime \prime} \mathrm{dm}^{3}  at equilibrium stage.V)   \mathrm{N}_{2}+3 \mathrm{H}_{2} \square  2 \mathrm{NH}_{3}

Q8 (a) Write down \mathrm{K}_{c} for the following reversible reactions. Suppose that the volume of reaction mixture in all the cases is V^{\prime \prime} \mathrm{dm}^{3} at equilibrium stage.V) \mathrm{N}_{2}+3 \mathrm{H}_{2} \square 2 \mathrm{NH}_{3}

ii) Which statement about the following equilibrium is correct 2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \square 2 \mathrm{SO}_{3}(\mathrm{~g}) \ddot{A} \mathrm{H}=-188.3 \mathrm{~kJ} \mathrm{~mol}{ }^{-1} (a) The value of K_{p} falls with a rise in temperature(b) The value of K_{p} falls with increasing pressure(c) Adding \mathrm{V}_{2} \mathrm{O}_{5} catalyst increase the equilibrium yield of sulphur trioxide(d) The value of K_{0} is equal to K_{\text {c. }} .
ii) Which statement about the following equilibrium is correct  2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \square 2 \mathrm{SO}_{3}(\mathrm{~g})   \ddot{A} \mathrm{H}=-188.3 \mathrm{~kJ} \mathrm{~mol}{ }^{-1} (a) The value of  K_{p}  falls with a rise in temperature(b) The value of  K_{p}  falls with increasing pressure(c) Adding  \mathrm{V}_{2} \mathrm{O}_{5}  catalyst increase the equilibrium yield of sulphur trioxide(d) The value of  K_{0}  is equal to  K_{\text {c. }} .

ii) Which statement about the following equilibrium is correct 2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \square 2 \mathrm{SO}_{3}(\mathrm{~g}) \ddot{A} \mathrm{H}=-188.3 \mathrm{~kJ} \mathrm{~mol}{ }^{-1} (a) The value of K_{p} falls with a rise in temperature(b) The value of K_{p} falls with increasing pressure(c) Adding \mathrm{V}_{2} \mathrm{O}_{5} catalyst increase the equilibrium yield of sulphur trioxide(d) The value of K_{0} is equal to K_{\text {c. }} .

Example:Calculate the \mathrm{pH} of a buffer solution in which 0.11 molar \mathrm{CH}_{3} \mathrm{COONa} and 0.09 molar acetic acid solutions are present. \mathrm{K}_{\mathrm{a}} for \mathrm{CH}_{3} \mathrm{COOH} is 1.85 \times 10^{-5}
Example:Calculate the  \mathrm{pH}  of a buffer solution in which  0.11  molar  \mathrm{CH}_{3} \mathrm{COONa}  and  0.09  molar acetic acid solutions are present.  \mathrm{K}_{\mathrm{a}}  for  \mathrm{CH}_{3} \mathrm{COOH}  is  1.85 \times 10^{-5}

Example:Calculate the \mathrm{pH} of a buffer solution in which 0.11 molar \mathrm{CH}_{3} \mathrm{COONa} and 0.09 molar acetic acid solutions are present. \mathrm{K}_{\mathrm{a}} for \mathrm{CH}_{3} \mathrm{COOH} is 1.85 \times 10^{-5}

1. For the decomposition of dinitrogen oxide \left(\mathrm{N}_{2} \mathrm{O}\right) into nitrogen and oxygen reversible reaction takes place as follows\[2 \mathrm{~N}_{2} \mathrm{O}_{(\mathrm{g})} \rightleftharpoons 2 \mathrm{~N}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}\]The concentration of \mathrm{N}_{2} \mathrm{O} \mathrm{N}_{2} and \mathrm{O}_{2} are 1.1 \mathrm{~mol} \mathrm{dm}^{-3} 3.90 \mathrm{~mol} \mathrm{dm}^{-3} and 1.95 \mathrm{~mol} \mathrm{dm}^{-3} respectively at equilibrium. Find out \mathrm{K}_{\mathrm{c}} for this reaction.
1. For the decomposition of dinitrogen oxide  \left(\mathrm{N}_{2} \mathrm{O}\right)  into nitrogen and oxygen reversible reaction takes place as follows\[2 \mathrm{~N}_{2} \mathrm{O}_{(\mathrm{g})} \rightleftharpoons 2 \mathrm{~N}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}\]The concentration of  \mathrm{N}_{2} \mathrm{O} \mathrm{N}_{2}  and  \mathrm{O}_{2}  are  1.1 \mathrm{~mol} \mathrm{dm}^{-3} 3.90 \mathrm{~mol} \mathrm{dm}^{-3}  and  1.95 \mathrm{~mol} \mathrm{dm}^{-3}  respectively at equilibrium. Find out  \mathrm{K}_{\mathrm{c}}  for this reaction.

1. For the decomposition of dinitrogen oxide \left(\mathrm{N}_{2} \mathrm{O}\right) into nitrogen and oxygen reversible reaction takes place as follows\[2 \mathrm{~N}_{2} \mathrm{O}_{(\mathrm{g})} \rightleftharpoons 2 \mathrm{~N}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}\]The concentration of \mathrm{N}_{2} \mathrm{O} \mathrm{N}_{2} and \mathrm{O}_{2} are 1.1 \mathrm{~mol} \mathrm{dm}^{-3} 3.90 \mathrm{~mol} \mathrm{dm}^{-3} and 1.95 \mathrm{~mol} \mathrm{dm}^{-3} respectively at equilibrium. Find out \mathrm{K}_{\mathrm{c}} for this reaction.

11. Write note on :(ii) dynamic equilibrium
11. Write note on :(ii) dynamic equilibrium

11. Write note on :(ii) dynamic equilibrium