The value of equilibrium constant for the given reaction needs to be determined. Concept introduction: The system is said to be in equilibrium if the there is no change in the partial pressure or concentration of reactant and product takes place. For a general reaction as follows: A ( g ) + B ( g ) ⇌ C ( g ) + D ( g ) The expression for the equilibrium constant is represented as follows: K = ( P C ) ( P D ) ( P A ) ( P B ) Here, to calculate the equilibrium constant, the values of partial pressure of all the species in reactant and product side are required. If an equilibrium reaction is reversed, the value of its equilibrium constant gets inversed. If an equilibrium reaction is multiplied by any value, the value will become the power of the equilibrium constant. On adding two equilibrium reactions, the value of their equilibrium constant gets multiplied. On subtracting two equilibrium reactions, the value of their equilibrium constant gets divided.
The value of equilibrium constant for the given reaction needs to be determined. Concept introduction: The system is said to be in equilibrium if the there is no change in the partial pressure or concentration of reactant and product takes place. For a general reaction as follows: A ( g ) + B ( g ) ⇌ C ( g ) + D ( g ) The expression for the equilibrium constant is represented as follows: K = ( P C ) ( P D ) ( P A ) ( P B ) Here, to calculate the equilibrium constant, the values of partial pressure of all the species in reactant and product side are required. If an equilibrium reaction is reversed, the value of its equilibrium constant gets inversed. If an equilibrium reaction is multiplied by any value, the value will become the power of the equilibrium constant. On adding two equilibrium reactions, the value of their equilibrium constant gets multiplied. On subtracting two equilibrium reactions, the value of their equilibrium constant gets divided.
Solution Summary: The author explains that the value of equilibrium constant for a given reaction needs to be determined.
The value of equilibrium constant for the given reaction needs to be determined.
Concept introduction:
The system is said to be in equilibrium if the there is no change in the partial pressure or concentration of reactant and product takes place.
For a general reaction as follows:
A(g)+B(g)⇌C(g)+D(g)
The expression for the equilibrium constant is represented as follows:
K=(PC)(PD)(PA)(PB)
Here, to calculate the equilibrium constant, the values of partial pressure of all the species in reactant and product side are required.
If an equilibrium reaction is reversed, the value of its equilibrium constant gets inversed. If an equilibrium reaction is multiplied by any value, the value will become the power of the equilibrium constant. On adding two equilibrium reactions, the value of their equilibrium constant gets multiplied. On subtracting two equilibrium reactions, the value of their equilibrium constant gets divided.
Consider the following reactions:
CO(g) + H20(g) +→CO2(g) + H2(g) K = 1.33 x 105
COlg) + 2 H2(g) +CH3OH(g) K2 = 2.59 x 107
Determine the value of the equilibrium constant for the following reaction:
CO2(3) + 3 H2(g) → CH3OH(g) + H2O(g)
A 1.00-L flask was filled with 2.00 moles of gaseous
SO2 and 2.00 moles of gaseous
NO2 and heated. After equilibrium was reached, it was found that 1.34 moles of gaseous
NO was present. Assume that the reaction
SO-(9) + NO2 (g) = SO; (g) + NO(9)
occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reaction.
K =
The equilibrium constant, Kc , for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g) is 6.90 x 103 .
(a) What is Kc for the reaction 2 SO3 (g) → 2 SO2 (g) + O2 (g)
(b) What is Kc for the reaction SO2 (g) + 1/2 O2 (g) → SO3 (g)