To calculate the value for the equilibrium constant Kp, we need to use the equilibrium pressures of the reactants and products.
Given:
PNO₂ = 0.55 atm
PNO = 6.5 × 10⁻⁵ atm
PO₂ = 4.5 × 10⁻⁵ atm
Since the reaction is 2NO₂ (g) ⇌ 2NO (g) + O₂ (g), the stoichiometric coefficients of the reactants and products are 2:2:1 respectively.
To calculate Kp, we need to use the following equation:
Kp = (PNO)² × (PO₂) / (PNO₂)²
Plugging in the given pressures, we have:
Kp = (6.5 × 10⁻⁵ atm)² × (4.5 × 10⁻⁵ atm) / (0.55 atm)²
Simplifying the equation, we get:
Kp = (4.225 × 10⁻⁹ atm²) × (2.025 × 10⁻⁹ atm) / (0.3025 atm²)
Kp = 8.55675 × 10⁻¹⁸ atm³ / 0.0917625 atm²
Kp = 9.3355 × 10⁻¹⁷ atm
Therefore, the value for the equilibrium constant Kp at this temperature is 9.3355 × 10⁻¹⁷ atm.
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Step-by-step explanation: