Consider the following chemical equilibrium: c(s) +2h2 (g) ch4 (g) now write an equation below that shows how to calculate from for this reaction at an absolute temperature . you can assume 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.

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.

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:

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

  the   balanced   equation   for   reaction of   ca metal   with   o2 to   produce   cao   is as below

2 ca+ o2→ 2 cao2

  explanation

the reaction is   balanced     since the   number of atoms   in reactant side is   equal to   number of atoms   in   product side.   for   example   they   are 2   atom of   ca in   reactant   side   and   2   atoms of ca   in   the product side.

  the   process   is a   meet the   requirement   of   redox   reaction because :     calcium   is   oxidized   from   oxidation state 0   to 2+   while   oxygen   is reduced from   oxidation   state   0   to 2-

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