Question

Consider the equilibrium system described by the chemical reaction below. A mixture of gas containing only N and H2is reacted in a vessel at high temperature. At equilibrium, the 5.0MH,8.0MN, and 4.0MNH, are present Determine the initial concentrations of H2and N, that were present in the vessel. N(g)+3H4( g)⇌2NH4( g) Based on the given values, fill in the ICE table to determine concentrations of all reactants and products.

Answer 1

To determine the initial concentrations of H2 and N in the vessel, we can use the ICE table. The initial concentration of N is approximately 1.6 M and the initial concentration of H2 is approximately 4.8 M.

Step-by-step explanation:

To determine the initial concentrations of H2 and N in the vessel, we can use the ICE table. The equation for the reaction is N(g) + 3H2(g) ⟷ 2NH3(g). At equilibrium, the concentrations of H2, N, and NH3 are 5.0 M, 8.0 M, and 4.0 M, respectively.

To fill in the ICE table, let's assume that the initial concentration of N is x and the initial concentration of H2 is 3x. Since the stoichiometric coefficients of N and H2 in the balanced equation are 1 and 3, respectively, we can determine the equilibrium concentrations using the equation:

8 - x = 4x

Solving for x gives us x ≈ 1.6 M. Therefore, the initial concentration of N is approximately 1.6 M and the initial concentration of H2 is approximately 3 * 1.6 M = 4.8 M.

Answer 2

To solve the problem, we used the ICE table based on the given equilibrium concentrations and chemical equation. We determined that the initial concentrations of N2 and H2 were 12.0M and 10.0M, respectively.

Step-by-step explanation:

To determine the initial concentration of H2 and N2 in the chemical reaction N(g)+3H2( g) ⇌ 2NH3( g) at high temperature, we need to utilize the Initial, Change, and Equilibrium (ICE) table which allows us to account changes in concentration through the progress of the chemical reaction.

Given that at equilibrium the concentrations are 5.0M H2, 8.0M N2, and 4.0M NH3. Since the reaction involves one molecule of N2 reacting with three molecules of H2 to form 2 molecules of NH3, the concentration changes are represented as:
N2: Initial = x, Change = -4.0M, Equilibrium = x - 4.0M = 8.0M
H2: Initial = y, Change = -5.0M, Equilibrium = y - 5.0M = 5.0M

From this, we can find that the initial concentrations of N2 and H2 were 12.0M and 10.0M, respectively.

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