Chemistry

Chemistry, 06.07.2019 08:30, zoolo1

Consider the reaction. at equilibrium, the concentrations of the different species are as follows. [nh3] = 0.105 m [n2] = 1.1 m [h2] = 1.50 m what is the equilibrium constant for the reaction at this temperature?

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Chemistry, 02.08.2019 20:10, Calirose

Calculate the equilibrium constant for the following two reactions. the equilibrium concentration of each reactant and product is given in the box below the reaction. rank the extent of each reaction at equilibrium by calculating the equilibrium constant. note that the "extent of each reaction" refers to how much reactant is converted to product at equilibrium. reaction 1: reaction 2: co(g)+o2(g)⇌2co2(g) 2n2(g)+o2(g)⇌2no2(g) equilibrium concentrations equilibrium concentrations [co]=1.3m [n2]=1.5m [o2]=1.3m [o2]=2.1m [co2]=8.8m [no2]=0.04m compare kc values to indicate which reaction proceeds to a greater extent at equilibrium. view available hint(s) compare values to indicate which reaction proceeds to a greater extent at equilibrium. reaction 2, with kc=45.8> reaction 1, with kc=3.4×10−4 reaction 1, with kc=5.21> reaction 2, with kc=1.3×10−2 reaction 2, with kc=3000> reaction 1, with kc=2.2×10−2 reaction 1, with kc=45.8> reaction 2, with kc=3.4×10−4

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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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