The equilibrium constant, Kc, for the following reaction is 10.5 at 350K. 2CH2Cl

Question

The equilibrium constant, Kc, for the following reaction is 10.5 at 350K. 2CH2Cl2(g) PCl3(g) + Cl2(g) If 0.163 moles of PCl5(g), 0.551 moles of PCl3, and 0.468 moles of Cl2 are at equilibrium in a 14.7 L container at 561 K, the value of the equilibrium constant, Kc, is___________ . CH4(g) + CCl4(g) If an equilibrium mixture of the three gases in a 17.1 L container at 350K contains 0.409 mol of CH2Cl2(g) and 0.470 mol of CH4, the equilibrium concentration of CCl4 is ___________ M. 2. Consider the following reaction: PCl5(g)

Explanation / Answer

K = [ ch4][ccl4]/[ch2cl2]^2

10.5 = [.47]*[ccl4]/[.409 ^2]

ccl4 = 3.73 moiles

   [ccl4] = 3.73/17.1

            .2185 M

2. Kc = [pcl3][cl2]/[pcl5]

          = [.551/14.7][.468/14.1]/[.163/14.7]

          = .107

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