Given that the enthalpy change of the reaction, Delta H = 18.8 kJ. So the reaction as written is endothermic. That is, heat is absorbed in the forward reaction.
According to Le Chatelier principle, any reaction at equilibrium when disturbed will act in a way to oppose the external disturbance.
As temperature is increased, the reaction will proceed in a direction in which the excess heat energy added is absorbed. As the forward reaction is endothermic, the excess heat energy will be absorbed if the forward reaction is dominant.
So as the temperature increases forward reaction takes place. Reactants concentration will decrease and products concentration will increase.
Ans: Concentration of CH2Cl2 will increase.
The reaction CH4 (8) + CCl4 (g) = 2 CH2Cl2 (B) has an enthalpy change AHI°...
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.
find the enthalpy change H for this reaction: CH4(g) + Cl2--> CCl4(g)+HCl Using the following Equations: C(s)+H2(g)-->CH4 H= -74.6 kJ C(s) + Cl2(g)--> CCl4 H=-95.7 kJ H2(g)+Cl2(g)--> HCl H=-92.3 kJ
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...
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
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
Predict and calculate the effect of temperature change on an equilibrium system. CHA reacts with CCl4 to form CH2Cl2. The equilibrium constant, Kp, for this reaction is 9.52x102 at 350 K. CH,(g) +CC1,0)=2CH,C1) The standard enthalpy change for this reaction (AH”) is 18.8 kJ/mol. (a) Predict the effect on the production of CH, Cl, when the temperature of the equilibrium system is increased. production is favored production is disfavored (6) Use the van't Hoff equation to estimate the equilibrium constant...
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, Kp, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) =CH4(g) + CCl4(g) If ΔH° for this reaction is -18.8 kJ, what is the value of Kp at 441 K? Kp =
A student ran the following reaction in the laboratory at 293 K: 2CH2Cl2(g) CH4(g) + CCl4(g) When she introduced 6.91×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(g) to be 3.19×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc=?
A student ran the following reaction in the laboratory at 283 K: 2CH2Cl2(g) ->CH4(g) + CCl4(g) When she introduced 7.70×10-2 moles of CH2Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of CCl4(g) to be 3.59×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc =