Chemistry

Chemistry, 22.06.2019 02:50, Jerrikasmith28

The conventional equilibrium constant expression (kc) for the system below is: 2icl(s) ⇄ i2(s) + cl2(g) [cl2] ([i2] + [cl2])/2[icl] [i2][cl2]/[icl]2 none of the listed answers are correct [i2][cl2]/2[icl]

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Chemistry, 29.08.2019 21:10, brittanylrodgers99

Circle the letter of the correct answer two answers are circled, and one of which is correct, half credit will be given 1125 pts 60 pts 1. which of the following statements concerning equilibrium is not true? a) a system that is disturbed from an equilibrium condition responds in a manner to restore equilibrium. b) equilibrium in molecular systems is dynamic with two opposing processes balancing one another c) the value of the equilibrium constant for a given reaction mixture is the same regardless of the direction from which equilibrium is attained d) a system moves spontaneously toward a state of equilibrium e) the equilibrium constant is independent of temperature 2. at a certain temperature. k = 25 and a reaction vessel contains a mixture with the following concentrations: h = 0.10 m brl - 0.10 mand thb 0.50 m which of the following statements concerning the reaction quotient, q. is true? h2(g) + br(g) =2hbr(g) a) q=k b) q ko more h2 and bra will be produced 3. the equilibrium constant for the decomposition of cobr2 is: cobra(9) co(g) + bra(g) k = 0.190 what is the value of kc for the following reaction? co(g) + bra(g) = cobra(9) a) 0.0361 b) 2.63 c) 5.26 d) 10.5 e) 27.7 calculate the 4. if the value for kp for the following reaction at 500 k is 1.5 x 10 value of the equilibrium constant, kc. n2(g) + 3h2(g) = 2nh3(g) c) 9.6 x 10-2 a) 7.5 x 10-2 d) 2.5 x 10-2 b) 1.3 x 10-2 e) 6.0 x 10-2

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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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