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) C(g) + D(g)
where Kc is equilibrium constant which is equal to the ratio of the concentrations of the product to reactants
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) 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 ?
- 0.29 atm
- 3.5 atm
- 0.53 atm
- 1.87 atm
The correct answer is: 0.29 atm
2SO2 (g) + O2(g) 2SO3 (g)
3.5 =
\ Partial pressure of O2 = 0.29 atm
Related Questions to study
Chemistry-
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) C(g) + D(g)
where Kc is equilibrium constant which is equal to the ratio of the concentrations of the product to reactants
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 KC for the reaction NOBr(g) from the following information at 298 K
2NO (g) N2 (g) + O2 (g) K1 = 2.4 × 1030
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) C(g) + D(g)
where Kc is equilibrium constant which is equal to the ratio of the concentrations of the product to reactants
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 KC for the reaction NOBr(g) from the following information at 298 K
2NO (g) N2 (g) + O2 (g) K1 = 2.4 × 1030
NOBr(g)K2 = 1.4
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