The reaction ${ 2A_{(g)} + B_{(g)} <=> 3C_{(g)} + D_{(g)}}$ is begun with the concentrations of $A$ and $B$ both at an intial value of $1.00\, M$. When equilibrium is reached, the concentration of $D$ is measured and found to be $0.25 \,M$. The value for the equilibrium constant for this reaction is given by the expression.
- $[(0.75)^3 (0.25)] \div [(0.50)^2 (0.75)]$
- $[(0.75)^3 (0.25)] \div [(0.50)^2 (0.25)]$
- $[(0.75)^3 (0.25)] \div [(0.75)^2 (0.25)]$
- $[(0.75)^3 (0.25)] \div [(1.00)^2 (1.00)]$
The Correct Option is A
Approach Solution - 1
The correct option is(A): \([(0.75)^3 (0.25)] \div [(0.50)^2 (0.75)]\)
Given,
(I)\(F{{e}_{2}}O(s)+3CO(g)\xrightarrow[{}]{{}}2Fe(s)+3C{{O}_{2}}(g);\)
\(\Delta H=-26.8\,\text{kJ}\)
(II)\(FeO(s)+CO(g)\xrightarrow[{}]{{}}Fe(s)+C{{O}_{2}}(g);\)
\(\Delta H=-16.5\,\text{kJ}\)
On multiplying Eq (II) with 2, we get
(III) \(2FeO(s)+2CO(g)\xrightarrow[{}]{{}}2Fe(s)+2C{{O}_{2}}(g);\)
\(\Delta H=-33\,\text{kJ}\)
On subtracting Eq (III) from I, we get
\(F{{e}_{2}}{{O}_{3}}(s)+CO(g)\xrightarrow[{}]{{}}2FeO(s)+C{{O}_{2}}(g);\)
\(\Delta H=-26.8-(-33)\)
\(=+6.2\,\text{kJ}\)
Approach Solution -2
Ans. Chemical equilibrium is the cThe number of integer value(s) of k for which the expression x^2-2(4k-1)x+15k^2 -2k-7>0 for every real number x is/areondition of a system in which the parameters of the system remain stable and neither the reactant concentration nor the product concentration changes over time. The system enters the condition of chemical equilibrium when the rate of the forward reaction equals the rate of the backward reaction. The system is said to be in a state of dynamic equilibrium if the concentrations of the reactants and products do not change further as a result of the equal rates of the forward and reverse processes.
Chemical equilibrium is the condition of a system where the concentrations of the reactant and the products do not fluctuate over time. The forward reaction rate and the reverse reaction rate are equal in a condition of chemical equilibrium. When the system reaches equilibrium, its characteristics do not show any further change.
A forethought is a graph with the time on the coordinate axis, usually known as the y-axis, and the concentration on the coordinate axis, commonly known as the x-axis. Chemical equilibrium is reached when the concentration of each reactant and product stops changing.
Chemical Equilibrium is helpful in several industrial processes like,
Preparation of Ammonia by Haber’s Process: In this N (nitrogen) combines with a chemical element to create ammonia, the yield of ammonia is a lot more at high temperatures, pressure, and within the presence of iron as a catalyst.
Preparation of Acid by Contacts Method: In this process, the elemental reaction is the chemical reaction of pollutants into sulfur oxide. This involves chemical equilibrium.
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Concepts Used:
Equilibrium
An equilibrium represents a state in a process when the observable properties such as color, temperature, pressure, concentration etc do not show any change.
The word equilibrium means ‘balance’ which indicates that a chemical reaction represents a balance between the reactants and products taking part in the reaction. The equilibrium state is also noticed in certain physical processes such as the melting point of ice at 0℃, both ice and water are present at equilibrium.
In the case of physical processes such as the melting of solid, dissolution of salt in water etc., the equilibrium is called physical equilibrium while the equilibrium associated with chemical reaction is known as chemical equilibrium.
Equilibrium in Chemical changes
The chemical equilibrium in a reversible reaction is the state at which both forward and backward reactions occur at the same speed.
The stage of the reversible reaction at which the concentration of the reactants and products do not change with time is called the equilibrium state.
Read More: Calculating Equilibrium Concentration
Types of Chemical Equilibrium
There are two types of chemical equilibrium:
- Homogeneous Equilibrium
- Heterogeneous Equilibrium
Homogenous Chemical Equilibrium
In this type, the reactants and the products of chemical equilibrium are all in the same phase. Homogenous equilibrium can be further divided into two types: Reactions in which the number of molecules of the products is equal to the number of molecules of the reactants. For example,
- H2 (g) + I2 (g) ⇌ 2HI (g)
- N2 (g) + O2 (g) ⇌ 2NO (g)
Reactions in which the number of molecules of the products is not equal to the total number of reactant molecules. For example,
- 2SO2 (g) + O2 (g) ⇌ 2SO3 (g)
- COCl2 (g) ⇌ CO (g) + Cl2 (g)
Heterogeneous Chemical Equilibrium
In this type, the reactants and the products of chemical equilibrium are present in different phases. A few examples of heterogeneous equilibrium are listed below.
- CO2 (g) + C (s) ⇌ 2CO (g)
- CaCO3 (s) ⇌ CaO (s) + CO2 (g)
Thus, the different types of chemical equilibrium are based on the phase of the reactants and products.
Check Out: Equilibrium Important Questions