Chemistry

Chemistry, 22.06.2019 01:00, deaishaajennings123

What is the equilibrium constant of aa+bb=cc+dd

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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.

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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Chemistry, 23.10.2019 23:00, Abrahamolve

How do the following changes affect the value of the equilibrium constant for a gas-phase exothermic reaction: 1) removal of a reactant. decrease equilibrium constant increase equilibrium constant no effect 2) removal of a product. increase equilibrium constant no effect decrease equilibrium constant 3) decrease in the volume no effect decrease equilibrium constant increase equilibrium constant 4) decrease in the temperature increase equilibrium constant no effect decrease equilibrium constant

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