Question 1 :
The value of K for a reaction can be changed by changing ____.<br/>
Question 2 :
To which type of reaction, Le Chatelier's principle can always be applied?
Question 3 :
The equilibrium constant K for the reaction:<br/>$2HI(g)\rightleftharpoons H_2(g)+I_1(g)$ at room temp is 2.85 and that at 698 K is $1.4\times 10^{-2}$. This implies that the forward reaction is:
Question 5 :
According to Le-Chatelier's principle, adding heat to a solid and liquid in equilibrium
Question 7 :
$\displaystyle 2NO\left( g \right) +{ H }_{ 2 }\left( g \right) \rightleftharpoons { N }_{ 2 }O\left( g \right) +{ H }_{ 2 }O\left( g \right) +351$kilojoules<br>If the total pressure on the system is increases when the reaction above is at equilibrium, which of the following occurs?
Question 8 :
Assertion: For a reaction $ H_2(g) + I_2(g) \rightleftharpoons 2HI(g) $ if the volume of vessel is reduced to half of its original volume , equilibrium constant will be doubled .
Reason: According to Le-Chaterlier principle , reaction shifts in a direction that tends to undo the effect of the stress .
Question 9 :
The yield of the products in the reaction, ${ A }_{ 2\left( g \right) }+2{ B }_{ \left( g \right) }\rightleftharpoons { C }_{ \left( g \right) }+Q$ $kJ$ would be higher at :
Question 10 :
For the reaction $2A \rightarrow B + 3C$; if $- \dfrac {d[A]}{dt} = k_{1}[A]^{2}; \dfrac {d[B]}{dt} = k_{2} [A]^{2}; \dfrac {d[C]}{dt} = k_{3}[A]^{2}$ the correct relation between $k_{1}, k_{2}$ and $k_{2}$ is:
Question 11 :
Which of the following equilibrium is not shifted by increase in the pressure?
Question 12 :
Assertion: As temperature increases, heat of reaction also increase for exothermic as well as endothermic reactions.
Reason: $\Delta { H }_{ reaction }$ varies according to the relation:<br><br>$\cfrac { \Delta { H }_{ 2 }-\Delta { H }_{ 1 } }{ { T }_{ 2 }-{ T }_{ 1 } } =\Delta { C }_{ P }$
Question 13 :
When a bottle of cold drink is opened, the gas comes out with a fizze due to :<br>
Question 14 :
$PCl_5(g) \rightleftharpoons Pcl_3(g)+Cl_2(g)$<br/>If more $Cl$ are added to the above reaction, how the equilibrium will be affected ?<br/>
Question 15 :
Increase in pressure favors formation of $HI$ from $H_{2}$ and $I_{2}$.<br/>
Question 16 :
Each of the following systems is at equilibrium in a closed container. A decrease in the total volume of each container increases the number of moles of product(s) for which system?
Question 17 :
The system $PCl_5(g)\rightleftharpoons PCl_3(g)+Cl_2(g)$ attains equilibrium. If the equilibrium concentration of $PCl_3(g)$ is doubled, the concentration of $Cl_2(g)$ would become:<br>
Question 18 :
In the reaction $N_2+O_2 \leftrightharpoons 2NO \ + $ heat, which of following conditions is suitable to get a good yield of $NO$?
Question 19 :
Assertion: When a catalyst is added to a reaction mixture in equilibrium, the amount of the products increases.
Reason: The forward reaction becomes faster/slower on adding the catalyst.
Question 20 :
Le- Chatelier's principle is applicable to both homogeneous and heterogeneous equilibria.
Question 22 : <div>In an equilibrium, the positive catalyst increases the rate of the forward reaction while decreases the rate of the backward reaction.<br/></div>
Question 23 :
Assertion: Ice $\rightleftharpoons $ water, if pressure is applied water will evaporate.
Reason: Increases of pressure pushes the equilibrium towards the side in which number of gaseous molecule increases.
Question 24 : The following reaction occurs in the Blast Furnace where ion ore is reduced to iron metal :<div><br/>$Fe_{2}O_{3}(s)+3CO(g)\rightleftharpoons 2Fe(l)+3CO(g)$</div><div><br/>Using Le Chatelier's principle, predict which of the following will not disturb the equilibrium?</div>
Question 25 :
The value of equilibrium constant for a reversible reaction is $3 \times 10^{-2}$. If the reaction quotient for the same reaction is $5 \times 10^{-3}$. Predict the direction of equilibrium reaction.
Question 27 :
When {tex} \mathrm { NaNO } _ { 3 } {/tex} is heated in a closed vessel, oxygen is liberated and {tex} \mathrm { NaNO } _ { 2 }{/tex} is left behind. At equilibrium.
Question 28 :
For the reversible reaction, $N_{2}(g) + 3H_{2}(g)\rightleftharpoons 2NH_{3}(g)$ at $500^{\circ}C$, the value of $K_{P}$ is $1.44\times 10^{-5}$ when partial pressure is measured in atmospheres. The corresponding value of $K_{C}$, with concentration in mole $litre^{-1}$, is
Question 29 :
For the gas phase reaction:<br>{tex} \mathrm { C } _ { 2 } \mathrm { H } _ { 4 } + \mathrm { H } _ { 2 } \rightleftharpoons \mathrm { C } _ { 2 } \mathrm { H } _ { 6 } ( \Delta \mathrm { H } = - 32.7 \mathrm { kcal } ) {/tex}<br>carried out in a vessel, the equilibrium concentration of {tex} \mathrm { C } _ { 2 } \mathrm { H } _ { 4 } {/tex} can be increased by :
Question 30 :
S : The red colour shown by $\left[{Fe\left(SCN\right)}\right]^{2+} \left(aq\right)$ in a reversible reaction between ${Fe}^{3+}$ and ${SCN}^{-}$.<br/> ${Fe}^{3+} \left(aq\right) + {SCN}^{-} \left(aq\right) \rightleftharpoons Fe{\left(SCN\right)}^{2+} \left(aq\right)$ deepens if few more drops of $KSCN$ are added in equilibrium mixture.<br/>E : Addition of $KSCN$ favours backward reaction.
Question 31 :
Which system at equilibrium will not be influenced by a change in pressure?
