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Complete Question:
Consider the following chemical equilibrium C(s) +2H2 (g) ⇄ CH4 (g) Now write an equation below that shows how to calculate Kp from Kc for this reaction at an absolute temperature T. You can assume T is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator.
Answer:
[tex]Kp = \frac{Kc}{R*T}[/tex]
Explanation:
Equilibrium occurs when the velocity of the formation of the products is equal to the velocity of the formation of the reactants at a reversible reaction. Because of that, the concentrations and the partial pressures of the substances remain constant.
The equilibrium can be characterized by the equilibrium constant, which is calculated by the activity of the substances. For solids and liquid water, activity is equal to 1. For liquids and aqueous substances, it is equal to the concentration, and for gases, it can be equal to the concentration or the partial pressure.
So, the constant can be calculated by the concentration (using liquid, aqueous and gases), and it's called Kc, or by pressure (using only gases substances), and it's called Kp. They're calculated by the multiplication of the concentration, or pressure, of the products (elevated by their coefficient) divided by the multiplication of the concentration, or pressure, of the reactants (elevated by their coefficient).
The constants are related by the equation:
[tex]Kp = Kc*(R*T)^{n}[/tex]
Where R is the gas constant, T is the temperature and n is the variation of the coefficients of the gas substances. So, for a generic reaction:
aA(g) + bB(g) ⇄ cC(g) + dD(g)
n = (a+b) - (c+d)
For the reaction given:
C(s) + 2H₂(g) ⇄ CH₄(g)
n = 2 - 1 = 1
Kp = Kc*(R*T)⁻¹
[tex]Kp = \frac{Kc}{R*T}[/tex]
- When Equilibrium occurs that when the velocity of the formation of the products is equal to the velocity of the formation of the reactants at a reversible reaction. Just Because of that, the concentrations and also the partial pressures of the substances remain constant.
- Also that The equilibrium can be characterized by the equilibrium constant, which is calculated by the activity of the substances. After that For solids and also that liquid water, which is activity is equal to 1. Now For liquids and also those aqueous substances, it is also equal to the concentration, and that for gases, it can be equal to the concentration or that is the partial pressure.
- So, When it is constant it can be calculated by the concentration (using liquid, aqueous, and gases), and also it's called Kc, They're also calculated by the multiplication of the concentration, which was or pressure, of the products (elevated by their coefficient) divided by the multiplication of the concentration, or pressure, of the reactants (elevated by their coefficient).
- Therefore The constants are related by the equation:
- Thus, that Where R is the gas constant when T is the temperature and also n is the variation of the coefficients of the gas substances. So, that it for a generic reaction:
- aA(g) + bB(g) ⇄ cC(g) + dD(g)
- n = (a+b) - (c+d)
- For the reaction given:
- C(s) + 2H₂(g) ⇄ CH₄(g)
- n = 2 - 1 = 1
- Kp = Kc*(R*T)⁻¹
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