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 |
Homework Answers
We first write balance equation. Accordingly we write concentration at equilibrium. And then write formula of Kc and put values in it. So CH2CL2 = 0.0399M
CH4 AND CCl4 = 0.9102M
Add Answer to:
34) The equilibrium constant, Kc, for the following
reaction is 10.5 at 350 K.
2CH2Cl2(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...
a) The equilibrium constant, Kc, for the following reaction is 9.52×10-2at 350 K. CH4(g) + CCl4(g)...
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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, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(8) CH4(8) +...
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(8) CH4(8) + CC14(8) Calculate the equilibrium concentrations of reactant and products when 0.242 moles of CH2Cl2 are introduced into a 1.00 L vessel at 350 K. M (CH2Cl2] [CH] [CC14] M M
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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
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
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 5.21×10-2 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
A) The equilibrium constant, Kc, for the following reaction is 10.5 at 350K. 2CH2Cl2(g) <->CH4(g) +...
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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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