# Equilibrium Constants

Equilibrium constants are fundamental concepts in chemical kinetics, providing crucial insights into the balance of reactants and products in a reversible reaction at equilibrium. Represented by the symbol K, these constants quantify the extent of a chemical reaction under specified conditions. They are essential in predicting the direction of a reaction and determining its equilibrium position. Understanding equilibrium constants is pivotal in various fields, including chemistry, biochemistry, and environmental science, as they help elucidate reaction dynamics and guide experimental design for optimal outcomes.

Questions

- What is the equilibrium constant for water?
- The #pKa# of butyric acid #"HBut"# is 4.7. How do you calculate #K_b# for the butyrate ion #"But"^-#?
- Consider the following reaction: #Xe(g) + 2F_2(g) -> XeF_4(g)#. A reaction mixture initially contains 2.24 atm #Xe# and 4.27 atm #F_2#. lf the equilibrium pressure of #Xe# is 0.34 atm, how do you find the equilibrium constant (#K_p#) for the reaction?
- How do you write the Keq equation?
- What is the equilibrium constant for the following reaction at #"298 K"#? And what is the partial pressure of #"S"_8(g)# above #"S"(s, "orthorhombic")# at equilibrium at #25^@ "C"#?
- At a certain temperature, 4.0 mol #NH_3# is introduced into a 2.0 L container, and the #NH_3# partially dissociates to #2NH_3(g)\rightleftharpoonsN_2(g)+3H_2(g)#. At equilibrium, 2.0 mol #NH_3# remains. What is the value of #K_c#?
- How do you calculate the Keq of a reaction?
- Write an equilibrium expression for each chemical equation involving one or more solid or liquid reactants or products #HCHO_(2(aq))+H_2O_((l))⇌H_3O_((aq))^(+)+CHO_(2(aq))^(-)#. Use A for #[HCHO_2]#, B for #[H_2O]#, C for #[H_3O^+]#, D for #[CHO_2^(−)]#?
- #H_2# (g) + #F_2# (g) #\rightleftharpoons2HF# (g), find final values of #[H_2]_(eq)#, #[F_2]_(eq)#, and #[HF]_(eq)#?
- What is the equilibrium constant expression for the equation #C(s) + O_2(g) rightleftharpoons CO_2(g)#?
- How do you solve #1.7xx10^(-1)=(x^2)/(0.60-x)# for #x#?
- What is the concentration of #"AlF"_6^"3-"# after mixing #"25 cm"^3# of 0.1 mol/L aluminium ion with #"25 cm"^3# of 1 mol/L fluoride ion?
- How is the value of the equilibrium constant useful?
- What is Kb and Ka in chemistry?
- How do you set up a Ksp equation?
- Why is keq unitless?
- At what approximate temperature will an equimolar mixture of #N_2(g)# and #O_2(g)# be 3.0 % converted to #NO(g)#?
- Why is it necessary to maintain a constant temperature in an experiment to measure an equilibrium constant?
- In the reaction #N_2(g) + 3H_2(g) -> 2NH_3(g)#, #N_2 = 10.00 M#, #H_2 = 8.00 M#, and #NH_3 = 2.00 M#. What is the equilibrium constant #K#, for this reaction?
- What is the equation for finding the equilibrium constant for a chemical reaction?