An experimenter places the following concentrations of gases in a closed container: NOBI]=0.245 M, [NO] = 3.29 x 10 M, Br2] = 2.02 x 10- M These%3Dgases then react:2NOB1(g) 2NO(g) + Br2 (g)4.At the temperature of the reaction, the equilibrium constant K, is 5.85 x 10 * Calculate the reaction quotient, Q, from the initial concentrations and determinewhether the concentration of NOBR increases or decreases as the reaction approaches equilibrium.Q.=%DThe concentration of NOBR

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An experimenter places the following concentrations of gases in a closed container: [NOB1] = 0.245 M, [NO] = 3.29 x 10M. Bra] = 2.02 x 10-3 M. These gases then react: 2NOBr(g) 2NO(9) + Br2 (g) At the temperature of the reaction, the equilibrium constant K. is 5.85 x 104. Calculate the reaction quotient, Q., from the initial concentrations and determine whether the concentration of NOBR increases or decreases as the reaction approaches equilibrium. Q. = of NOB

An experimenter places the following concentrations of gases in a closed container: [NOB1] = 0.245 M, [NO] = 3.29 x 10M. Bra] = 2.02 x 10-3 M. These gases then react: 2NOBr(g) 2NO(9) + Br2 (g) At the temperature of the reaction, the equilibrium constant K. is 5.85 x 104. Calculate the reaction quotient, Q., from the initial concentrations and determine whether the concentration of NOBR increases or decreases as the reaction approaches equilibrium. Q. = of NOB

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 50P

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