For the same reaction and temperature as in Worked Example 15.11, calculate the equilibrium concentrations of all three species if the starting concentrations are as follows: [H2] = 0.00623 M, [I2] = 0.00414 M, and [HI] = 0.0424 M.
Interpretation:
The HI equilibrium constant (Kc) values should be calculated given the respective molar concentration of reactants and products at
Concept Introduction:
Equilibrium constant (K): Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.
Homogeneous equilibrium: A homogeneous equilibrium involved has an everything present in the same phase and same conditions, for example reactions where everything is a gas, or everything is present in the same solution.
Equilibrium concentration: If Kc and the initial concentration for a reaction and calculate for both equilibrium concentration, and using the (ICE) chart and equilibrium constant and derived changes in respective reactants and products.
Answer to Problem 15.12WE
The equilibrium concentration (Kc) value is given the hydrogen iodide chemical reaction is showed below.
Explanation of Solution
To find: Calculate the each
First we calculate the equilibrium table to determine the equilibrium concentrations of each species in terms of unknown (x) then solve for (x) and use it to calculate the equilibrium molar concentrations.
Let us consider the given equilibrium concentration values, to substitute (Kc) equation we get the equilibrium constant values.
The equilibrium concentration values are
The equal moles of H2 and I2 reacted in gas phase conditions to give 2 moles of HI, the balance equation are showed above. Then the depletion in the concentration of HI at equilibrium, the equilibrium concentration of H2 and I2 consider as (x), the calculation methods showed the table.
The HI molar concentration is derived given the equilibrium concentration (Kc) and its reaction.
Want to see more full solutions like this?
Chapter 15 Solutions
Loose Leaf For Chemistry: Atoms First With Connect 2y Access Card
- For the following system, K=4.86105 at 298K: HClO(aq)+F(aq)ClO(aq)+HF(aq) Assuming that you start with equal concentrations of HClO and F, and that no ClO or HF is initially present, which of the following best describes the equilibrium system: a the forward reaction is favored at equilibrium; b the reverse reaction is favored at equilibrium; c appreciable quantities of all species are present at equilibrium?arrow_forwardWrite the equilibrium constant expression for each reaction in terms of activities, simplifying where appropriate. a C(s)+O2(g)CO2(g) b P4(s)+5O2(g)P4O10(s) c 2HNO2(g)+3Cl2(g)2NCl3(g)+H2(g)+2O2(g)arrow_forward. Ammonia. a very important industrial chemical. is produced by the direct combination of the following elements under carefully controlled conditions: N2(g)+3H2(g)2NH3(g)Suppose. in an experiment, that the reaction mixture is analyzed after equilibrium is reached, and it is found, at a particular temperature. that [NH3]=0.25M,[H2]=3.4103M, and [N2]=5.3105M. Calculate the value of K at this temperature.arrow_forward
- Solid CaCO3 ; is placed in a closed container and heated to 800 °C. What is the equilibrium concentration of Co2 in the following equilibrium, for which K=2.5103 ? CaCO3(s)CaO(s)+Co2(g)arrow_forwardIsopropyl alcohol is the main ingredient in rubbing alcohol. It can decompose into acetone (the main ingredient in nail polish remover) and hydrogen gas according to the following reaction: C3H7OH(g)C2H6CO(g)+H2(g)At 180C, the equilibrium constant for the decomposition is 0.45. If 20.0 mL (d=0.785g/mL) of isopropyl alcohol is placed in a 5.00-L vessel and heated to 180C, what percent- age remains undissociated at equilibrium?arrow_forward5.16. In atmospheric chemistry, the following chemical reaction converts , the predominant oxide of sulfur that comes from combustion of S-containing materials, to , which can combine with to make sulfuric acid (and thus contribute to acid rain): (a) Write the expression for K for this equilibrium. (b) Calculate the value of for this equilibrium using the values in Appendix 2. (c) Calculate the value of K for this equilibrium. (d) If of and of are enclosed in a system in the presence of some liquid, in which direction would the reaction move?arrow_forward
- Colorless hydrogen gas (H2) and red-brown colored bromine gas (Br2) reacts to form colorless HBr gas. Describe how the concentrations of H2, Br2, and HBr would change increase or decrease as equilibrium was established in a sealed container that initially contained only H2 and Br2. What observation would indicate that equilibrium had been established?arrow_forward. Suppose that for a hypothetical reaction: A2(g)+2B(g)2AB(g)It is determined that at a certain temperature the equilibrium concentrations are: [A2]=0.0090,[B]=0.940, and [AB]=5.3104. Calculate the numerical value of K for the reaction.arrow_forward. Gaseous phosphorus pentachloride decomposes according to the reaction PCl5(g)PCl3(g)+Cl2(g)The equilibrium system was analyzed at a particular temperature, and the concentrations of the substances present were determined to be [PCl5]=1.1102M,[PCl3]=0.325M. and [Cl2]=3.9103M. Calculate the value of K for the reaction.arrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemical Principles in the LaboratoryChemistryISBN:9781305264434Author:Emil Slowinski, Wayne C. Wolsey, Robert RossiPublisher:Brooks Cole
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningPhysical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning