Interpretation:
The value of equilibrium constant
Concept introduction:
The acids that do not undergo complete dissociation when dissolved in water are known as weak acids. The equilibrium constant in the case of dissociation of a weak acid is known as the acid constant and is denoted by
Answer to Problem 19PE
The value of equilibrium constant
Explanation of Solution
The equilibrium reaction is shown below.
The volume of the reaction chamber is
The formula to calculate the molar concentration of the compounds is given below.
Substitute the value of initial number of moles of
Substitute the value of initial number of moles of
Substitute the value of final number of moles of
The change in concentration of
Substitute the values of final and initial concentrations of
The negative sign indicates that the concentration of
According to the equilibrium reaction,
The ICE table for the given reaction is shown below.
The value of
Substitute the values of concentrations of
Therefore, the value of
The value of equilibrium constant
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Chapter 18 Solutions
Introductory Chemistry: An Active Learning Approach
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- At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?arrow_forwardConsider the system 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H20(ℓ) ΔrH° = −1530.4 kJ/mol How will the amount of ammonia at equilibrium be affected by removing O2(g) without changing the total gas volume? adding N2(g) without changing the total gas volume? adding water without changing the total gas volume? expanding the container? increasing the temperature? Which of these changes (i to v) increases the value of K? Which decreases it?arrow_forward
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