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Answer to Question #63428 in General Chemistry for S
Question #63428
Chapter 15 (15.87)
At 700 K the equilibrium constant for the reaction
CCl4(g)←−→C(s)+2Cl2(g)
is Kp=0.76. A flask is charged with 2.00 atm of CCl4, which then reaches equilibrium at 700 K.
1) What fraction of the CCl4 is converted into C and Cl2?
2) What is the partial pressure of CCl4 at equilibrium?
3) What is the partial pressure of Cl2 at equilibrium?
At 700 K the equilibrium constant for the reaction
CCl4(g)←−→C(s)+2Cl2(g)
is Kp=0.76. A flask is charged with 2.00 atm of CCl4, which then reaches equilibrium at 700 K.
1) What fraction of the CCl4 is converted into C and Cl2?
2) What is the partial pressure of CCl4 at equilibrium?
3) What is the partial pressure of Cl2 at equilibrium?
Expert's answer
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