Tetrafluoroethene, C:F4, is obtained from chlorodifluoromethane, CHCIF:, accordingto the equation:2CHCIF: (g) = C:F+ (g) + 2HC1(g)AH = +128 kJ m olA 1.0 mol sample of CHCIF2 is placed in a container of volume 18.5 L andheated. When equilibrium is reached, the mixture contains 0.20 mol of CHCIF2.(a) Calculate the number of moles of C:F4 and the number of moles of HClpresent at equilibrium.(b) Calculate a value for Kc and give its units.

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o the equation: 2CHCIF: (g)=C:F+ (g) + 2HC1(g) AH® = +128 kJ m ol A 1.0 mol sample of CHCIF: is placed in a container of volume 18.5 L and neated. When equilibrium is reached, the mixture contains 0.20 mol of CHCIF:. a) Calculate the number of moles of C:F. and the number of moles of HCl present at equilibrium. b) Calculate a value for Kc and give its units.

o the equation: 2CHCIF: (g)=C:F+ (g) + 2HC1(g) AH® = +128 kJ m ol A 1.0 mol sample of CHCIF: is placed in a container of volume 18.5 L and neated. When equilibrium is reached, the mixture contains 0.20 mol of CHCIF:. a) Calculate the number of moles of C:F. and the number of moles of HCl present at equilibrium. b) Calculate a value for Kc and give its units.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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