17.5 mm #2
The following gas phase system is at equilibrium:
CCl4(g) + CH4(g) ⇄ 2
CH2Cl2(g)
The pressure of each gas is measured at 301
K:
P(CCl4) = 173 mmHg
P(CH4) = 1.72×10-3
mmHg
P(CH2Cl2) = 113 mmHg
What is the Gibbs free energy change at this temperature?
kJ/mol
17.5 mm #2 The following gas phase system is at equilibrium: CCl4(g) + CH4(g) ⇄ 2...
The reaction CH4 (8) + CCl4 (g) = 2 CH2Cl2 (B) has an enthalpy change AHI° - 18.8 kJ. You allow the equation to proceed to equilibrium at 25 °C, then raise the temperature to 50 °C. How will the equilibrium concentrations be affected by this temperature change? Concentrations of CH4 and CCl4 will increase. Concentration of CH2Cl2 will increase. Concentrations of CCl4 and CH2Cl2 will increase The concentrations will remain the same.
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 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) -> 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...
Consider the following system at equilibrium where Kc = 9.52×10-2 and H° = 18.8 kJ/mol at 350 K. CH4 (g) + CCl4 (g) goes to 2 CH2Cl2 (g) The production of CH2Cl2 (g) is favored by: Indicate True (T) or False (F) for each of the following: 1. decreasing the temperature. 2. decreasing the pressure (by changing the volume). 3. increasing the volume. 4. removing CH2Cl2 . 5. removing CCl4 .
Consider the following system at equilibrium where K. = 9.52x10-2 and AH° = 18.8 kJ/mol at 350 K. CH4 (g) + CCl4 (g) – 2 CH2Cl2 (g) The production of CH2Cl2 (g) is favored by: Indicate True (T) or False (F) for each of the following: - 1. decreasing the temperature. 2. decreasing the pressure (by changing the volume). 3. increasing the volume. 4. adding CH2Cl2 - 5. adding CC14 -
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 5.21×10-2 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
Consider the following system at equilibrium at 350 K: 2CH2Cl2(g) CH4(g) + CCl4(g) When some CH4(g) is removed from the equilibrium system at constant temperature: The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of CCl4 will: A. Increase. B. Decrease. C. Remain the same.
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?