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 |
Homework Answers
Answer:-
This question is solved by using simple concept of chemical equilibrium. Firstly equilibrium constant expression is written then using the its value equilibrium concentration is calculated.
The answer is given in the image,
Add Answer to:
The equilibrium constant, Kc, for the following
reaction is 9.52×10-2 at
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)...
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The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 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] =
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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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
The equilibrium constant, Kc, for the following reaction is 37.9 at 292 K. 2CH2Cl2(g) CH4(g) +...
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