The following reaction 2H2S(g) = 2H2(g) + S2(g), Ke=1.67 × 10-7 at 800°C is carried out at 800 °C with the following initial concentrations: H2S] = 0.100M, [H2] = 0.100M, and [S2] = 0.00 M. Find the equilibrium concentration of S2. Express the molarity to three significant figures.
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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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![### Chemical Equilibrium Analysis
#### Example Reaction and Condition Setup
Consider the following reaction:
\[ 2H_2S(g) \rightleftharpoons 2H_2(g) + S_2(g) \]
with the given equilibrium constant:
\[ K_c = 1.67 \times 10^{-7} \text{ at } 800^\circ\text{C} \]
#### Initial Conditions
This reaction is conducted at \( 800^\circ\text{C} \) with the initial concentrations:
\[ [H_2S] = 0.100 \, M \]
\[ [H_2] = 0.100 \, M \]
\[ [S_2] = 0.00 \, M \]
#### Problem Statement
Find the equilibrium concentration of \( S_2 \).
**Requirements:**
- Express the molarity to three significant figures.
#### Input Area
A text box is provided for entering the calculated equilibrium concentration of \( S_2 \):
\[ [S_2]_{eq} = \boxed{\phantom{M}} \, M \]
This setup helps in understanding how to determine the equilibrium concentrations of the substances involved in the reaction, given initial conditions and the reaction’s equilibrium constant.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fca24ea45-8ee9-42f4-b908-77c9ffd9f0e0%2F19d9afd5-f625-44b9-b968-a3b667b23787%2Fodyxes7_processed.jpeg&w=3840&q=75)
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