A student ran the following reaction in the laboratory at 282 K:2CH2C12(g)=CH4(g)+ CCI4(g)When she introduced 6.98x102 moles of CH,Ch(g) into a 1.00 liter container, she found the equilibrium concentration of CH,Cl2(g) to be 4.62x10³ M.Calculate the equilibrium constant, K, she obtained for this reaction.K. =

Given data,Initial moles of CH2Cl2=6.98×10-2molVolume of container=1.0LEquilibrium concentration of…

A student ran the following reaction in the laboratory at 282 K: 2CH,Cl½(g) CH4(g) + CC14(g) When she introduced 6.98×10-² moles of CH,Cl(g) into a 1.00 liter container, she found the equilibrium concentration of CH,Cl2(g) to be 4.62×103 M. Calculate the equilibrium constant, K., she obtained for this reaction. K. =

A student ran the following reaction in the laboratory at 282 K: 2CH,Cl½(g) CH4(g) + CC14(g) When she introduced 6.98×10-² moles of CH,Cl(g) into a 1.00 liter container, she found the equilibrium concentration of CH,Cl2(g) to be 4.62×103 M. Calculate the equilibrium constant, K., she obtained for this reaction. K. =

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 60QRT

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