A sample of carbon is placed in a rigid 1.50 L flask. Dinitrogen monoxide is added and the flask heated to 800C. When the system reached equilibrium the partial pressure of the carbon dioxide is found to be 0.030 atm and the partial pressure of the dinitrogen monoxide to be 1.48 atm. What is the value of the equilibrium constant, Kp for the system at 800C?
The value of
1. Write the balanced chemical equation for the equilibrium.
C(s) + 2N₂O(g) ⇌ CO₂(g) + 2N₂(g)
2. Write the
3 List the equilibrium concentrations. There was no According to the equation, the reaction forms twice as much 4. Insert these values into the
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To calculate the equilibrium constant ( K_p ) for the system at 800°C, we use the equation:
[ K_p = \frac{{P_{\text{{CO}}2}}}{{P{\text{{N}}_2\text{{O}}}}} ]
Substitute the given partial pressures:
[ K_p = \frac{{0.030 , \text{{atm}}}}{{1.48 , \text{{atm}}}} ]
[ K_p \approx 0.0203 ]
So, the equilibrium constant ( K_p ) for the system at 800°C is approximately 0.0203.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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