Chemistry, 09.11.2019 18:31, cecelia090

Consider the reaction. mc032-1.jpg at equilibrium, the concentrations of the different species are as follows. [h2o] = 0.077 m [cl2o] = 0.077 m [hclo] = 0.023 m what is the equilibrium constant for the reaction at this temperature?

0.089
0.26
3.9
11

Answers: 3

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Chemistry, 07.07.2019 16:30, youngcie04

Consider the reaction.at equilibrium, the concentrations of the different species are as follows.[h2o] = 0.077 m[cl2o] = 0.077 m[hclo] = 0.023 mwhat is the equilibrium constant for the reaction at this temperature? 0.0890.263.911

Answers: 1

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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.

Answers: 1

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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.

Answers: 3

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Chemistry, 09.10.2019 22:00, kingk7368

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] = 0.800 m , and [c] = 0.500 m . the following reaction occurs and equilibrium is established: a+2b⇌c at equilibrium, [a] = 0.150 m and [c] = 0.700 m . calculate the value of the equilibrium constant, kc. express your answer numerically.

Answers: 3

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Consider the reaction. mc032-1.jpg at equilibrium, the concentrations of the different species are as follows. [h2o] = 0.077 m [cl2o] = 0.077 m [hclo] = 0.023 m what is the equilibrium constant for the reaction at this temperature? 0.089 0.26 3.9 11

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Consider the reaction. mc032-1.jpg at equilibrium, the concentrations of the different species are as follows. [h2o] = 0.077 m [cl2o] = 0.077 m [hclo] = 0.023 m what is the equilibrium constant for the reaction at this temperature?

0.089
0.26
3.9
11