The equilibrium constant, Kc, for the following reaction is 41.1 at 289 K. 2CH2Cl2(g) --> CH4(g) + CCl4(g)Â Â When a...

60.1K

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Chemistry

The equilibrium constant, K_c, for the followingreaction is 41.1 at 289 K.

2CH₂Cl₂(g)--> CH₄(g) +CCl₄(g)Â Â

When a sufficiently large sample ofCH₂Cl₂(g) is introduced intoan evacuated vessel at 289 K, the equilibriumconcentration of CCl₄(g) is found to be0.202 M.Â Â

Calculate the concentration ofCH₂Cl₂ in the equilibriummixture. ? M
2)The equilibrium constant, K_c, for the followingreaction is 1.80Ã—10^-2 at698 K.Â Â
Calculate K_p for this reaction at thistemperature.Â Â

2HI(g) -->H₂(g)+Â Â I₂(g)
3) The equilibrium constant, K_c, for the followingreaction is 5.10Ã—10^-6 at548 K.Â Â
Calculate K_p for this reaction at thistemperature.Â Â

NH₄Cl(s) -->NH₃(g)+Â Â HCl(g)

Answer & Explanation Solved by verified expert

3.6 Ratings (557 Votes)

Let us write ICE table for the equilibrium reaction 2CH2Cl2g CH4g CCl4g I a moles 0 0 C x moles x2 x2 E ax x2 x2 Note It is assumed that before equilibrium reached x moles of CH2Cl2 dissociates Since the Stocihiometric ratio See Answer

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