Tetrafluoroethene, C2F4, is obtained from chlorodifluoromethane, CHClF2, according to the equation: 2CHClF2 (g) C2F4 (g) + 2HCl(g) A 1.0 mol sample of CHClF2 is placed in a container of volume 18.5 L and heated. When equilibrium is reached, the mixture contains 0.20 mol of CHClF2. (a) Calculate the number of moles of C2F4 and the number of moles of HCl present at equilibrium. (b) Calculate a value for Kc and give its units.
Tetrafluoroethene, C2F4, is obtained from chlorodifluoromethane, CHClF2, according to the equation: 2CHClF2 (g) C2F4 (g) + 2HCl(g) A 1.0 mol sample of CHClF2 is placed in a container of volume 18.5 L and heated. When equilibrium is reached, the mixture contains 0.20 mol of CHClF2. (a) Calculate the number of moles of C2F4 and the number of moles of HCl present at equilibrium. (b) Calculate a value for Kc and give its units.
Chapter16: Applications Of Neutralization Titrations
Section: Chapter Questions
Problem 16.2QAP
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Tetrafluoroethene, C2F4, is obtained from chlorodifluoromethane, CHClF2, according to the equation:
2CHClF2 (g) C2F4 (g) + 2HCl(g)
A 1.0 mol sample of CHClF2 is placed in a container of volume 18.5 L and
heated. When equilibrium is reached, the mixture contains 0.20 mol of CHClF2.
(a) Calculate the number of moles of C2F4 and the number of moles of HCl present at equilibrium.
(b) Calculate a value for Kc and give its units.
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