Consider the following reaction where Kc = 10.5 at 350 K: 2CH2Cl2(g) <=> CH4(g) + CCl4(g)...
Consider the following reaction where Kc = 10.5 at 350 K:
2CH2Cl2(g) <=> CH4(g) + CCl4(g)
A reaction mixture was found to contain 1.13×10-2 moles of CH2Cl2(g), 2.50×10-2moles of CH4(g) , and 4.11×10-2 moles of CCl4(g) in a 1.00 liter container.
Is the reaction at equilibrium?
If not, what direction must it run in order to reach equilibrium?
The reaction quotient, Qc = ____________
The reaction: ________
A. must run in the forward direction to reach equilibrium
B. must run in the reverse direction to reach equilibrium
C. is at equilibrium
(Enter numbers as numbers, no units. For example, 300 minutes would be 300. For letters, enter A, B, or C. Enter numbers in scientific notation using e# format. For example 1.43×10-4 would be 1.43e-4.)
Homework Answers
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Consider the following reaction where Kc = 10.5 at
350 K:
2CH2Cl2(g) <=> CH4(g) +
CCl4(g)...
The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) = CH4(g)...
The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) = CH4(g) + CCl4(g) Calculate the equilibrium concentrations of reactant and products when 0.294 moles of CH2Cl2 are introduced into a 1.00 L vessel at 350 K. [CH2Cl2] = ? M [CH4] = ? M [CCl4] = ? M
The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) >>CH4(g) +...
The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) >>CH4(g) + CCl4(g) Calculate the equilibrium concentrations of reactant and products when 0.327 moles of CH2Cl2 are introduced into a 1.00 L vessel at 350 K. [CH2Cl2] = M [CH4] = M [CCl4] = M The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) >>CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.275 moles of COCl2(g) are...
34) The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) <--->...
34) The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) <---> CH4(g) + CCl4(g) Calculate the equilibrium concentrations of reactant and products when 0.222 moles of CH2Cl2 are introduced into a 1.00 L vessel at 350K. [CH2Cl2] = ___ M [CH4] = ___ M [CCl4] = ___ M
The equilibrium constant, Kc, for the following reaction is 9.52×10-2 at 350 K: CH4(g) + CCl4(g)...
The equilibrium constant, Kc, for the following reaction is 9.52×10-2 at 350 K: CH4(g) + CCl4(g) <---> 2CH2Cl2(g) Calculate the equilibrium concentrations of reactants and product when 0.343 moles of CH4 and 0.343 moles of CCl4 are introduced into a 1.00 L vessel at 350 K. [CH4] = M [CCl4] = M [CH2Cl2] = M
a) The equilibrium constant, Kc, for the following reaction is 9.52×10-2at 350 K. CH4(g) + CCl4(g)...
a) The equilibrium constant, Kc, for the following reaction is 9.52×10-2at 350 K. CH4(g) + CCl4(g) -> 2 CH2Cl2(g) Calculate the equilibrium concentrations of reactants and product when 0.251 moles ofCH4and 0.251 moles of CCl4are introduced into a 1.00 L vessel at 350 K. [ CH4] = M [ CCl4] = M [ CH2Cl2] = M b) The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500 K. PCl5(g) ->PCl3(g) + Cl2(g) Calculate the equilibrium concentrations of reactant...
A) The equilibrium constant, Kc, for the following reaction is 10.5 at 350K. 2CH2Cl2(g) <->CH4(g) +...
A) The equilibrium constant, Kc, for the following reaction is 10.5 at 350K. 2CH2Cl2(g) <->CH4(g) + CCl4(g) If an equilibrium mixture of the three gases in a 19.9 L container at 350K contains 0.416 mol of CH2Cl2(g) and 0.202 mol of CH4, the equilibrium concentration of CCl4 is B) 2SO3(g) <->2SO2(g) + O2(g) If 0.184 moles of SO3(g), 0.477 moles of SO2, and 0.234 moles of O2 are at equilibrium in a 15.0 L container at 1.23×103 K, the value...
A student ran the following reaction in the laboratory at 293 K: 2CH2Cl2(g) CH4(g) + CCl4(g)...
A student ran the following reaction in the laboratory at 293 K: 2CH2Cl2(g) CH4(g) + CCl4(g) When she introduced 6.91×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(g) to be 3.19×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc=?
A student ran the following reaction in the laboratory at 283 K: 2CH2Cl2(g) ->CH4(g) + CCl4(g) ...
A student ran the following reaction in the laboratory at 283 K: 2CH2Cl2(g) ->CH4(g) + CCl4(g) When she introduced 7.70×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(g) to be 3.59×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g)----> CH4(g) + CCl4(g) An equilib...
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g)----> CH4(g) + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.59×10-2 M CH2Cl2, 0.181 M CH4 and 0.181 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.134 mol of CCl4(g) is added to the flask? [CH2Cl2] = _____ M [CH4] = _____ M [CCl4] = _____ M
1. The equilibrium constant, Kc, for the following reaction is 42.2 at 288 K. 2CH2Cl2(g) <----->...
1. The equilibrium constant, Kc, for the following reaction is 42.2 at 288 K. 2CH2Cl2(g) <-----> CH4(g) + CCl4(g) When a sufficiently large sample of CH2Cl2(g) is introduced into an evacuated vessel at 288 K, the equilibrium concentration of CCl4(g) is found to be 0.140 M. Calculate the concentration of CH2Cl2 in the equilibrium mixture. _____ M 2. A student ran the following reaction in the laboratory at 295 K: 2CH2Cl2(g) <-------> CH4(g) + CCl4(g) When she introduced 8.46×10-2 moles...
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