A student ran the following reaction in the laboratory at 332 K: 2CH2Cl2(g) ---->CH4(g) + CCl4(g) When she introduced
Posted: Thu Feb 17, 2022 11:14 am
A student ran the following reaction in the laboratory
at 332 K:
2CH2Cl2(g)
---->CH4(g)
+ CCl4(g)
When she
introduced CH2Cl2(g) at
a pressure of 0.455 atm into a 1.00 L
evacuated container, she found the equilibrium partial
pressure of CCl4(g) to
be 0.201 atm.
Calculate the equilibrium constant, Kp, she
obtained for this reaction.
Kp =
at 332 K:
2CH2Cl2(g)
---->CH4(g)
+ CCl4(g)
When she
introduced CH2Cl2(g) at
a pressure of 0.455 atm into a 1.00 L
evacuated container, she found the equilibrium partial
pressure of CCl4(g) to
be 0.201 atm.
Calculate the equilibrium constant, Kp, she
obtained for this reaction.
Kp =