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 of the
equilibrium constant, Kc, is
Homework Answers
Add Answer to:
A)
The equilibrium constant, Kc, for the following reaction
is 10.5 at 350K.
2CH2Cl2(g)
<->CH4(g) +...
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 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...
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...
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) CH4(g) +...
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 5.09E-2 M CH2Cl2, 0.165 M CH4 and 0.165 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.82E-2 mol of CH2Cl2(g) is added to the flask? [CH2Cl2] = M [CH4] = M [CCl4] = M
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) CH4(g) +...
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 5.21×10-2 M CH2Cl2, 0.169 M CH4 and 0.169 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.139 mol of CCl4(g) is added to the flask? [CH2Cl2] = M [CH4] = M [CCl4] = M
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) = CH4(g)...
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) = CH4(g) + CC14(9) Calculate the equilibrium concentrations of reactant and products when 0.377 moles of CH,Cl2 are introduced into a 1.00 L vessel at 350 K (CH2Cl2] = [CH4] = [CCl4] =
The equilibrium constant, Kc, for the following reaction is 37.9 at 292 K. 2CH2Cl2(g) CH4(g) +...
The equilibrium constant, Kc, for the following reaction is 37.9 at 292 K. 2CH2Cl2(g) CH4(g) + CCl4(g) When a sufficiently large sample of CH2Cl2(g) is introduced into an evacuated vessel at 292 K, the equilibrium concentration of CCl4(g) is found to be 0.492 M. Calculate the concentration of CH2Cl2 in the equilibrium mixture._______ 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...
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) = CH4(g) + CC14(9) Calculate the equilibrium concentrations of reactant and products when 0.377 moles of CH,Cl2 are introduced into a 1.00 L vessel at 350 K (CH2Cl2] = [CH4] = [CCl4] =
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