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Chemistry-

General

Easy

Question

If the composition of the system does not change with time, the system is said to be in chemical equilibrium. It is the state in which net reaction of a system is zero. In another words we can say that in reversible reactions, a stage is reached when the rate of transformation of reactants into products equals to the rate of transformation of products into reactants. At this stage, the composition of reactants and products does not change with time. This does not mean that the reaction has ceased, as both reverse and forward reactions are still taking place but with equal rate. Such equilibria are called dynamic equilirbria.
Let us consider a reaction of the type
A (g) + B(g) $Error converting from MathML to accessible text.$ C(g) + D(g)
$K subscript C end subscript equals fraction numerator open square brackets C close square brackets open square brackets D close square brackets over denominator open square brackets A close square brackets open square brackets B close square brackets end fraction$
where Kc is equilibrium constant which is equal to the ratio of the concentrations of the product to reactants
$K subscript P end subscript equals fraction numerator P subscript C end subscript cross times P subscript D end subscript over denominator P subscript A end subscript cross times P subscript B end subscript end fraction$
where KP is the equilibrium constant which is equal to the ratio of partial pressure of products to reactants. The relation between KP and KC is as follows.
KP = Kc(RT)^Dⁿ
20.For the reaction
NH2COONH4(s) $Error converting from MathML to accessible text.$ 2 NH3(g) + CO2(g)
The equilibrium constant KP = 2.9 × 10-5 atm3. The total pressure of gases at equilibrium when mole of reactant was heated will be

0.0194 atm
0.0388 atm
0.0580 atm
0.0667 atm

The correct answer is: 0.0580 atm

Related Questions to study

If the composition of the system does not change with time, the system is said to be in chemical equilibrium. It is the state in which net reaction of a system is zero. In another words we can say that in reversible reactions, a stage is reached when the rate of transformation of reactants into products equals to the rate of transformation of products into reactants. At this stage, the composition of reactants and products does not change with time. This does not mean that the reaction has ceased, as both reverse and forward reactions are still taking place but with equal rate. Such equilibria are called dynamic equilirbria.
Let us consider a reaction of the type
A (g) + B(g) $Error converting from MathML to accessible text.$ C(g) + D(g)
$Error converting from MathML to accessible text.$
where Kc is equilibrium constant which is equal to the ratio of the concentrations of the product to reactants
$Error converting from MathML to accessible text.$
where KP is the equilibrium constant which is equal to the ratio of partial pressure of products to reactants. The relation between KP and KC is as follows.
KP = Kc(RT)^Dⁿ
The equilibrium constant for the reaction 2 SO2(g) + O2(g) $Error converting from MathML to accessible text.$ 2 SO3(g) at 1000 K is 3.5. What would the partial pressure of oxygen gas if there are equal moles of SO2 and SO3 ?

If the composition of the system does not change with time, the system is said to be in chemical equilibrium. It is the state in which net reaction of a system is zero. In another words we can say that in reversible reactions, a stage is reached when the rate of transformation of reactants into products equals to the rate of transformation of products into reactants. At this stage, the composition of reactants and products does not change with time. This does not mean that the reaction has ceased, as both reverse and forward reactions are still taking place but with equal rate. Such equilibria are called dynamic equilirbria.
Let us consider a reaction of the type
A (g) + B(g) $Error converting from MathML to accessible text.$ C(g) + D(g)
$Error converting from MathML to accessible text.$
where Kc is equilibrium constant which is equal to the ratio of the concentrations of the product to reactants
$Error converting from MathML to accessible text.$
where KP is the equilibrium constant which is equal to the ratio of partial pressure of products to reactants. The relation between KP and KC is as follows.
KP = Kc(RT)^Dⁿ
The equilibrium constant for the reaction 2 SO2(g) + O2(g) $Error converting from MathML to accessible text.$ 2 SO3(g) at 1000 K is 3.5. What would the partial pressure of oxygen gas if there are equal moles of SO2 and SO3 ?

Chemistry-General

If the composition of the system does not change with time, the system is said to be in chemical equilibrium. It is the state in which net reaction of a system is zero. In another words we can say that in reversible reactions, a stage is reached when the rate of transformation of reactants into products equals to the rate of transformation of products into reactants. At this stage, the composition of reactants and products does not change with time. This does not mean that the reaction has ceased, as both reverse and forward reactions are still taking place but with equal rate. Such equilibria are called dynamic equilirbria.
Let us consider a reaction of the type
A (g) + B(g) $Error converting from MathML to accessible text.$ C(g) + D(g)
$Error converting from MathML to accessible text.$
where Kc is equilibrium constant which is equal to the ratio of the concentrations of the product to reactants
$Error converting from MathML to accessible text.$
where KP is the equilibrium constant which is equal to the ratio of partial pressure of products to reactants. The relation between KP and KC is as follows.
KP = Kc(RT)^Dⁿ
Determine K_C for the reaction $Error converting from MathML to accessible text.$ $Error converting from MathML to accessible text.$ NOBr(g) from the following information at 298 K
2NO (g) $Error converting from MathML to accessible text.$ N2 (g) + O2 (g) K1 = 2.4 × 1030
$Error converting from MathML to accessible text.$ $Error converting from MathML to accessible text.$ NOBr(g)K2 = 1.4

If the composition of the system does not change with time, the system is said to be in chemical equilibrium. It is the state in which net reaction of a system is zero. In another words we can say that in reversible reactions, a stage is reached when the rate of transformation of reactants into products equals to the rate of transformation of products into reactants. At this stage, the composition of reactants and products does not change with time. This does not mean that the reaction has ceased, as both reverse and forward reactions are still taking place but with equal rate. Such equilibria are called dynamic equilirbria.
Let us consider a reaction of the type
A (g) + B(g) $Error converting from MathML to accessible text.$ C(g) + D(g)
$Error converting from MathML to accessible text.$
where Kc is equilibrium constant which is equal to the ratio of the concentrations of the product to reactants
$Error converting from MathML to accessible text.$
where KP is the equilibrium constant which is equal to the ratio of partial pressure of products to reactants. The relation between KP and KC is as follows.
KP = Kc(RT)^Dⁿ
Determine K_C for the reaction $Error converting from MathML to accessible text.$ $Error converting from MathML to accessible text.$ NOBr(g) from the following information at 298 K
2NO (g) $Error converting from MathML to accessible text.$ N2 (g) + O2 (g) K1 = 2.4 × 1030
$Error converting from MathML to accessible text.$ $Error converting from MathML to accessible text.$ NOBr(g)K2 = 1.4

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