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The following equilibrium pressures at a certain temperature were observed for the reaction 2NO₂ (g)⇌2NO(g)+O₂ (g) PNO₂=0.55atm PNO=6.5×10⁻⁵atm PO₂=4.5×1⁻⁵atm Calculate the value for the equilibrium constant Kp at this temperature

User Nahomie
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1 Answer

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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.

Please let me know if there's anything else I can help you with.

Step-by-step explanation:

User Jan Pisl
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