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Answer to Question #71624 in General Chemistry for Anonymous
Question #71624
At 700 K the equilibrium constant for the reaction
CCl4(g)←−→C(s)+2Cl2(g)
is Kp=0.76. A flask is charged with 1.90 atm of CCl4, which then reaches equilibrium at 700 K. What fraction of the CCl4 is converted into C and Cl2?
CCl4(g)←−→C(s)+2Cl2(g)
is Kp=0.76. A flask is charged with 1.90 atm of CCl4, which then reaches equilibrium at 700 K. What fraction of the CCl4 is converted into C and Cl2?
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