Chemistry

Chemistry, 14.09.2019 06:30, avalonr2003

The value of the equilibrium constant for the following chemical equation is kr 40 at 25°c. calculate the solubility of al(oh)s(s) in an aqueous solution buffered at ph 11.00 at 25°c. al(oh)(s)oh (aq)al(oh)l'(aq) + a) 4.0 x 1010 m b) 6.3 m d) 0.37 m c) 0.040 m

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Chemistry, 20.09.2019 17:20, wcraig1998

Learning goal: to understand how to calculate the equilibrium constants for chemical equations that can be produced by the addition of other chemical equations with known equilibrium constants. for a chemical reaction equation with the general form aa+bb⇌cc+dd the equilibrium equation is given by k1 =[c]c[d]d[a]a[b]b thus, for a chemical reaction equation with the general form cc+dd⇌ee+ff the equilibrium equation is given by k2=[e]e[f]f[c]c[d]d if the first two equations are added together such that aa+bb⇌ee+ff then the equilibrium equation is given by k3 =[e]e[f]f[a]a[b]b=[c]c[d]d[a]a[b]b⋅[e]e[f]f[c]c[d]d or k3=k1⋅k2 thus, when a chemical equation is the sum of two chemical equations for which equilibrium constants are already known, the equilibrium constant for the reaction is the product of the equilibrium constants for the individual reactions. keep in mind that equilibrium equations do not include expressions for any pure solids or liquids that may be involved in the reaction. part a given the two reactions h2s⇌hs−+h+, k1 = 9.35×10−8, and hs−⇌s2−+h+, k2 = 1.59×10−19, what is the equilibrium constant kfinal for the following reaction? s2−+2h+⇌h2s enter your answer numerically. view available hint(s)

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Chemistry, 20.09.2019 19:30, GabriellaDul

At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, kc, which is a mathematical expression based on the chemical equation. for example, in the reaction aa+bb⇌cc+dd where a, b, c, and d are the stoichiometric coefficients, the equilibrium constant is kc=[c]c[d]d[a]a[b]b where [a], [b], [c], and [d] are the equilibrium concentrations. if the reaction is not at equilibrium, the quantity can still be calculated, but it is called the reaction quotient, qc, instead of the equilibrium constant, kc. qc=[c]tc[d]td[a]ta[b]tb where each concentration is measured at some arbitrary time t. part a a mixture initially contains a, b, and c in the following concentrations: [a] = 0.300 m , [b] = 1.10 m , and [c] = 0.450 m . the following reaction occurs and equilibrium is established: a+2b⇌c at equilibrium, [a] = 0.110 m and [c] = 0.640 m . calculate the value of the equilibrium constant, kc. express your answer numerically.

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Chemistry, 21.09.2019 23:30, kyriejr

At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, kc, which is a mathematical expression based on the chemical equation. for example, in the reaction aa+bb⇌cc+dd where a, b, c, and d are the stoichiometric coefficients, the equilibrium constant is kc=[c]c[d]d[a]a[b]b where [a], [b], [c], and [d] are the equilibrium concentrations. if the reaction is not at equilibrium, the quantity can still be calculated, but it is called the reaction quotient, qc, instead of the equilibrium constant, kc. qc=[c]tc[d]td[a]ta[b]tb where each concentration is measured at some arbitrary time t. part a a mixture initially contains a, b, and c in the following concentrations: [a] = 0.350 m , [b] = 0.750 m , and [c] = 0.350 m . the following reaction occurs and equilibrium is established: a+2b⇌c at equilibrium, [a] = 0.150 m and [c] = 0.550 m . calculate the value of the equilibrium constant, kc. express your answer numerically.

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