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In a chemical reaction. A(s)+B(g) C(g) the total pressure at equilibrium is 6 atm. The value of equilibrium constant is: (a) 2 (b) 9 (c) 1 (d) 36?
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In a chemical reaction. A(s)+B(g) C(g) the total pressure at equili...
Explanation:
Given:
- Chemical reaction: A(s) + B(g) → C(g)
- Total pressure at equilibrium = 6 atm
Calculating the equilibrium constant:
- The equilibrium constant (Kp) for the given reaction can be calculated using the formula:
Kp = (PC)^c / (PA)^a * (PB)^b
Where a, b, and c are the stoichiometric coefficients of A, B, and C in the balanced chemical equation.
Given that the total pressure at equilibrium is 6 atm:
- Let's assume that the partial pressures of A, B, and C at equilibrium are PA, PB, and PC respectively.
- Since A is in solid state, its partial pressure is considered to be constant and can be taken as 1 atm.
- Therefore, PB + PC = 6 atm
Substitute the values in the equilibrium constant expression:
Kp = PC / (1)(PB)
Kp = PC / PB
Given that the total pressure at equilibrium is 6 atm:
- Substitute PB = 6 - PC in the equation above:
Kp = PC / (6 - PC)
At equilibrium, the total pressure is 6 atm:
- This implies that PC + PB = 6
- Substitute PB = 6 - PC in the equation above:
PC + (6 - PC) = 6
6 = 6
Therefore, the equilibrium constant (Kp) for the given reaction is:
Kp = PC / (6 - PC)
Kp = 6 / (6 - 6)
Kp = 6 / 0
Kp = Undefined
Conclusion:
- The equilibrium constant for the given reaction cannot be determined with the provided information.
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In a chemical reaction. A(s)+B(g) C(g) the total pressure at equilibrium is 6 atm. The value of equilibrium constant is: (a) 2 (b) 9 (c) 1 (d) 36?
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