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) + 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) + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.39×10-2 M CH2Cl2, 0.175 M CH4 and 0.175 M CCl4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.118 mol of CCl4(g) is added to the flask?
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
6) Distrubuting Equilibrium a) 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 5.32x10-2 M CH2C2, 0.172 M CH4 and 0.172 M CCI4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 9.58x102 mol of CH4(g is added to the flask? CH2Cl2l [CH4 [CCI4] b) The equilibrium constant, K, for the...
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, 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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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, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) > CH4(g) + CCl4(g) Calculate the equilibrium partial pressures of all species when CH2Cl2(g) is introduced into an evacuated flask at a pressure of 0.939 atm at 350 K. PCH2Cl2 = atm PCH4 = atm PCCl4 = atm
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...