If the pressure of \[{{N}_{2}}/{{H}_{2}}\] mixture in a closed apparatus is 100 atm and 20% of the mixture then reacts, the pressure at the same temperature will be:
The exothermic formation of \[Cl{{F}_{3}}\] is represented by the equation: \[C{{l}_{2(g)}}+3{{F}_{2(g)}}\rightleftharpoons 2Cl{{F}_{3(g)}}\]; \[\Delta H=-329\,KJ\] Which of the following will increase the quantity to \[Cl{{F}_{3}}\] in an equilibrium mixture of\[C{{l}_{2}},\,{{F}_{2}}\] and \[Cl{{F}_{3}}\]?
For the equilibrium, \[CuS{{O}_{4}}\cdot 5{{H}_{2}}O(s)\]\[CuS{{O}_{4}}\cdot 3{{H}_{2}}O(s)+2{{H}_{2}}O(g),\] \[{{K}_{p}}=1.086\times {{10}^{-4}}\,at{{m}^{-2}}\] at \[25{}^\circ C\]. The efflorescent nature of \[CuS{{O}_{4}}\cdot 5{{H}_{2}}O\,(s)\] can be noticed when the vapour pressure of water in the atmosphere is (in mm Hg)
For the reaction \[A(g)+2B(g)\rightleftharpoons C(g)+D(g);{{K}_{C}}={{10}^{12}}.\] If the initial moles of A, B, C and D are 0.5, 1, 0.5 and 3.5 moles respectively in a one litre vessel. What is the equilibrium concentration of B?
The equilibrium constant for the reaction: \[{{N}_{2(g)}}+{{O}_{2(g)}}\rightleftharpoons 2N{{O}_{(g)}}\] is \[4\times {{10}^{-4}}\] at 200 K. In the presence of a catalyst, the equilibrium is attained 10 times faster. Therefore, the equilibrium constant in the presence of the catalyst at 200 K is:
\[A{{B}_{3}}(g)\] is dissociation as \[A{{B}_{3}}(g)A{{B}_{2}}(g)+\frac{1}{2}{{B}_{2}}(g),\] When the initial pressure of \[A{{B}_{3}}\] is 800 torr and the total pressure developed at equilibrium is 900 torr. What fraction of \[A{{B}_{3}}(g)\] is dissociated?
At a certain temperature the equilibrium constant \[{{K}_{c}}\] is 0.25 for the reaction \[{{A}_{2}}(g)+{{B}_{2}}(g){{C}_{2}}(g)+{{D}_{2}}(g),\] If we take 1 mole of each of the four gases in a 10 litre container, what would be equilibrium concentration of \[{{A}_{2}}(g)\]?
A system at equilibrium is described by the equation of fixed temperature T. \[S{{O}_{2}}C{{l}_{2}}(g)S{{O}_{2}}(g)+C{{l}_{2}}(g)\] What effect will an increases in the total pressure caused by a decrease in volume have on the equilibrium?
A)
Concentration of \[S{{O}_{2}}C{{l}_{2}}(g)\] increases
For the reaction at 300 K \[A(g)V(g)+S(g)\] \[{{\Delta }_{r}}{{H}^{{}^\circ }}=-30\,kJ/mol,\,\,\,{{\Delta }_{r}}{{S}^{{}^\circ }}=-0.1kJ.\,\,{{K}^{-1}}.\,\,mo{{l}^{-1}}\] What is the value of equilibrium constant?
In the following reaction: \[2S{{O}_{2}}(g)+{{O}_{2}}(g)2S{{O}_{3}}(g)\] the equilibrium is not attained. The rate of forward reaction is greater than that of backward reaction. Thus, which of the following is the correct relation between \[{{K}_{p}}\] and \[{{Q}_{p}}\]?
When \[{{N}_{2}}{{O}_{5}}\] is heated at temperature T, it dissociates as \[{{N}_{2}}{{O}_{5}}(g)\rightleftharpoons {{N}_{2}}{{O}_{3}}(g)+{{O}_{2}}(g),\] \[{{K}_{c}}=2.5.\] At the same time \[{{N}_{2}}{{O}_{3}}\] decomposes as \[{{N}_{2}}{{O}_{3}}(g)\rightleftharpoons {{N}_{2}}O(g)+{{O}_{2}}(g).\] If initially 4.0 moles of \[{{N}_{2}}{{O}_{5}}\] are taken in 2.0 litre flask and allowed to attain equilibrium, concentration of \[{{O}_{2}}\] was formed to be 2.5 M. Equilibrium concentration of \[{{N}_{2}}O\] is -
The value of \[{{K}_{C}}\] for the reaction \[{{N}_{2}}(g)+3{{H}_{2}}(g)\rightleftharpoons 2N{{H}_{3}}(g)\] is 0.50 at \[{{400}^{o}}C\]. What will be the value of \[{{K}_{p}}\] at \[{{400}^{o}}C\] when concentrations are expressed in mol \[{{L}^{-1}}\] and pressure in atmosphere?
The decomposition reaction \[PC{{l}_{5}}(g)\rightleftharpoons PC{{l}_{3}}(g)+C{{l}_{2}}(g)\] has \[{{K}_{c}}=0.245\text{M}\] at \[\text{30}{{\text{0}}^{o}}C\]. What happens in a container which contains the three gases each at a concentration of 0.3 M?
A)
the concentration of \[C{{l}_{2}}(g)\] and \[PC{{l}_{5}}(g)\] increases and that of \[PC{{l}_{3}}(g)\] decreases
doneclear
B)
the concentration of \[PC{{l}_{3}}(g)\] and \[C{{l}_{2}}(g)\] increases and that of \[PC{{l}_{5}}(g)\] decreases
doneclear
C)
the concentration of \[PC{{l}_{3}}(g)\] and \[PC{{l}_{5}}(g)\] increases and that of \[C{{l}_{2}}(g)\] decreases
doneclear
D)
the concentration of \[PC{{l}_{5}}(g)\] increases and those of \[PC{{l}_{3}}(g)\] and decreases \[C{{l}_{2}}(g)\]
The reaction \[CaC{{O}_{3}}\left( s \right)\rightleftharpoons CaO\left( s \right)+C{{O}_{2}}\left( g \right)\] is taking place in such a way that the vapour pressure of \[C{{O}_{2}}\] is equal to atmospheric pressure therefore, which of the following is not correct
The equilibrium constant K for the reaction \[2H{{I}_{(g)}}\rightleftharpoons {{H}_{2(g)}}+{{I}_{2(g)}}\] at room temperature is 2.85 and that at 698 K is \[1.4\times {{10}^{-2}}\]. This implies that:
A)
HI is an exothermic compound
doneclear
B)
HI is very stable at room temperature
doneclear
C)
HI is relatively less stable than \[{{H}_{2}}\] and \[{{I}_{2}}\]
\[{{H}_{2}}(g)+{{I}_{2}}(g)2HI(g)\] When 46g of \[{{I}_{2}}\] and 1g of \[{{H}_{2}}\] are heated at equilibrium at \[450{}^\circ C,\] the equilibrium mixture contained 1.9 g of of \[{{I}_{2}}\]. How many moles of \[{{I}_{2}}\] and HI are present at equilibrium?
At temperature T, a compound \[A{{B}_{2(g)}}\] dissociates according to the reaction\[2A{{B}_{2(g)}}2A{{B}_{(g)}}+{{B}_{2(g)}}\] with a degree of dissociation x, which is small compared with unity. The expression for \[{{K}_{p}},\] in terms of x and the total pressure, P is
For the reaction \[A+BC+D,\]equilibrium concentration of [C] =[D] = 0.5M if we start with 1 mole each of A and B. Percentage of A converted into C if we start with 2 moles of A and 1 mole of B, is
The equilibrium constant \[{{K}_{c}}\] for the reaction \[{{P}_{4}}(g)2{{P}_{2}}(g)\] is 1.4 at \[400{}^\circ C.\] Suppose that 3 moles of \[{{P}_{4}}(g)\] and 2 moles of \[{{P}_{2}}(g)\] are mixed in 2 litre container at \[400{}^\circ C.\]. What is the value of reaction quotient (Q)?
\[=\frac{2/3}{2}=\frac{1}{3}=0.33\] Ammonium carbonate dissociates as \[N{{H}_{2}}COON{{H}_{4}}(s)2N{{H}_{3}}(g)+C{{O}_{2}}(g)\] in a closed vessel containing ammonium carbamate in equilibrium. Ammonia is added such that partial pressure of \[N{{H}_{3}}\] now becomes two times to the equilibrium pressure. Calculate the ratio of partial pressure of \[C{{O}_{2}}\] now to the original partial pressure of \[C{{O}_{2}}\].
For gaseous decomposition of\[PC{{l}_{5}}\], in a closed vessel the degree of dissociation \['\alpha '\], equilibrium pressure 'P' &\[{{K}_{p}}\] are related as
One mole of nitrogen and three moles of hydrogen are mixed in a 4 litre container. If 0.25 percent of nitrogen is converted to ammonia by the following reaction - \[{{N}_{2}}(g)+3{{H}_{2}}(g)\rightleftharpoons 2N{{H}_{3}}(g)\] what will be the value of K for the following equilibrium? \[{{N}_{2}}(g)+3{{H}_{2}}(g)\rightleftharpoons 2N{{H}_{3}}(g)\] \[\frac{1}{2}{{N}_{2}}(g)+\frac{3}{2}{{H}_{2}}(g)\rightleftharpoons N{{H}_{3}}(g).\]
One mole of a compound AB reacts with one mole of a compound CD according to the equation \[A{{B}_{(g)}}+C{{D}_{(g)}}A{{D}_{(g)}}+C{{B}_{(g)}}.\]When equilibrium had been established it was found that 3/4 mole each of reactants AB and CD had been converted to AD and CB. There is no change in volume. The equilibrium constant for the reaction is
A mixture of nitrogen and hydrogen in the ratio of 1 : 3 reach equilibrium with ammonia when 50% of the mixture has reacted. If the total pressure is p, the partial pressure of ammonia in the equilibrium mixture was
For a chemical reaction at equilibrium the value of degree of dissociation is given by\[\alpha =\frac{{{M}_{t}}-{{M}_{0}}}{{{M}_{0}}(n-1)}\]. For this equation to be applicable pick out the incorrect statement.
