Question

Consider the following chemical equilibrium:

N2(g) + 3H2(g) ⇌ 2NH3

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.

Answer 1

To calculate the equilibrium constant (K) for the reaction of nitrogen and hydrogen to form ammonia at a given temperature, use the equilibrium concentrations in the formula K = [NH3]^2/([N2][H2]^3).

Step-by-step explanation:

To calculator the equilibrium constant (K) for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) at a specific absolute temperature, you can use the concentrations of the gases at equilibrium.

The general expression for the equilibrium constant (K) for this reaction is K = [NH3]^2/([N2][H2]^3), where the square brackets denote the molarity (concentration in moles per liter) of each species when the reaction is at equilibrium. To find the value of K at a given temperature, plug in the equilibrium concentrations of the reactants and products into this formula.

For example, if at 500 °C the equilibrium concentrations are 1.35 M H2, 1.15 M N2, and 4.12 x 10−1 M NH3, you would calculate K as follows:

K = [4.12 x 10−1]^2 / ([1.15][1.35]^3)

It's important to note that K is temperature dependent, and the values at various temperatures given (e.g., K25°C 3.3 × 109, K177°C 2.6 × 103, K327°C 4.1) indicate that the position of equilibrium shifts with changes in temperature.

Answer 2

Step-by-step explanation:

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Question

Asked Sep 26, 2019

Consider the following chemical equilibrium:

N2(g) + 3H2(g) ⇌ 2NH3(g)

Now write an equation below that shows how to calculate Kc from Kp 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.

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Expert Answer

Step 1

A reversible chemical reaction can move in either forward or backward direction. The stage of a reversible reaction at which the rate of forward and backward reaction become equal to each other is called an equilibrium stage.

Step 2

The equilibrium constant for a reaction is the ratio of equilibrium concentration of product and reactant. If the reaction is given in gaseous state, then the equilibrium pressure must be considered.

Step 3

The Keq expression for the answer is attached