Question

In: Chemistry

Multiple Part Question. For the reaction at 25C CCL4(l) + H2(g) -> HCl(g) + CHCl3(l) Delta...

Multiple Part Question.

For the reaction at 25C

CCL4(l) + H2(g) -> HCl(g) + CHCl3(l) Delta H°= -21.83 kcal and delta S°= 9.92 cal/K What is the delta G° for the reaction?

What is the value of Delta G in kcal mol-1 for the reaction taking place above if pH2 =10.0 atm and pHCL = .100 atm?

What is the equilibrium constant for the reaction described above at 25° C?

Solutions

Expert Solution

Reaction:   

---------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------The special name given to the equilibrium constant for the dissolving of an ionic solute in water is the solubility product constant or simply solubility product. It is denoted by.

Given chemical reaction is

The expression for equilibrium constant is:

Calculate equilibrium constant for the above reaction is as follows:

--------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------

----------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------


Related Solutions

2) Consider the equation: CHCl3(g) + Cl2(g)  CCl4(g) + HCl(g) The initial rate of reaction...
2) Consider the equation: CHCl3(g) + Cl2(g)  CCl4(g) + HCl(g) The initial rate of reaction is measured at several different concentrations of the reactants with the following results From the data, determine: a. the rate law for the reaction b. the rate constant (k) for the reaction CHCl3 Cl2 rate M/s 0.125 M 0.100 M 0.0025 M/s 0.250 M 0.100 M 0.0100 M/s 0.250 M 0.200 M 0.0200 M/s
Consider the following reaction: H2(g) +Br2(g) <=> 2HBr(g) Kc=2.0x10^9 at 25C If 0.100 mol H2 and...
Consider the following reaction: H2(g) +Br2(g) <=> 2HBr(g) Kc=2.0x10^9 at 25C If 0.100 mol H2 and 0.200 mol of Br2 were placed in a 10.0L container at 25C, what will the equilibrium concentrations of H2, Br2 and HBr be?
A mixture was prepared that contained 50.0 g of CCl4 and 50.0 g of CHCl3. At...
A mixture was prepared that contained 50.0 g of CCl4 and 50.0 g of CHCl3. At 50 C, the vapor pressure of pure CCl4 is 317 torr and that of CHCl3 is 526 torr. What is the vapor pressure of this mixture at 50 C?
Chloroform, CHCl3, is formed by the following reaction: CH4(g) + 3 Cl2(g) → 3 HCl(g) +...
Chloroform, CHCl3, is formed by the following reaction: CH4(g) + 3 Cl2(g) → 3 HCl(g) + CHCl3 (g) Determine the enthalpy change for this reaction (ΔH°rxn), using the following: enthalpy of formation of CHCl3 (g), ΔH°f = – 103.1 kJ/mol                                 CH4(g) + 2 O2(g) → 2 H2O(l) + CO2(g)        ΔH°rxn = – 890.4 kJ/mol                                 2 HCl (g) → H2 (g) + Cl2(g)                              ΔH°rxn = + 184.6 kJ/mol                                 C (graphite) + O2(g) → CO2(g)                     ΔH°rxn = – 393.5 kJ/mol                                 H2 (g)...
Consider the following reaction at 298 K: C(graphite)+2CL(g)------> CCl4(l) delta H=-139 kj Calculate delta S sys...
Consider the following reaction at 298 K: C(graphite)+2CL(g)------> CCl4(l) delta H=-139 kj Calculate delta S sys delta S surr delta S univ
Consider the reaction: Zn(s) + 2 H+(aq) = Zn2+(aq) + H2(g) At 25C, calculate: a) ∆G˚...
Consider the reaction: Zn(s) + 2 H+(aq) = Zn2+(aq) + H2(g) At 25C, calculate: a) ∆G˚ for the reaction, given that: ∆Gf Zn(s) = 0, ∆Gf(H+) = 0, ∆Gf(H2) = 0, ∆Gf(Zn2+) = -147.1 kj/mol b) ∆G, when P(h2) = 750 mmHg, [Zn2+ aq] = 0.10 M, [H+] = 1.0 x 10^-4 M c) The pH when ∆G - -100 kJ, P(h2) = 0.922 atm, [Zn2+] = 0.200 M and the mass of Zn is 155 g.
A 0.1002 g sample containing only CCl4 and CHCl3 was dissolved in methanol and electrolyzed at...
A 0.1002 g sample containing only CCl4 and CHCl3 was dissolved in methanol and electrolyzed at the surface of a mercury electrode at –1.0 V, which required 50.20 s at a constant current of 0.200 A. The potential of the cathode was then adjusted and held constant at –1.80 V. Completion of the titration at this potential required 382.35 s at a constant current of 0.200 A. Calculate the respective percentages of CCl4 and CHCl3 in the mixture. The electrolysis...
Reaction of HCl (aq) and Mg(s) to form MgCl2(aq) and H2(g) Given: Molarity of HCL :...
Reaction of HCl (aq) and Mg(s) to form MgCl2(aq) and H2(g) Given: Molarity of HCL : 3.00M volume of HCL: 20.0mL mass of Mg: 0.036g volume of gas before placing in equalization chamber: 37.0mL volume of gas after placing in equalization chamber: 37.5 mL barometric pressure of the room: 736.4 mmhg temperature of the room: 18.5 C ------------------------------------------------ Calculate: mole of Mg reacted: mole of H2(g) formed: vapor pressure of vater: pressure of H2 (Daltons Law): pressure of H2 in...
Calculate delta H for the reaction H(g) + Br(g) = HBr(g), given the following information: H2(g)...
Calculate delta H for the reaction H(g) + Br(g) = HBr(g), given the following information: H2(g) + Br2(g) = 2HBr(g) delta H = -72 kJ H2(g) = 2H(g) delta H = +436 kJ Br2(g)= 2Br(g) delta H = +224 kJ
Consider the following gas-phase reaction: C2H2(g) + 4 Cl2(g) 2 CCl4(g) + H2(g) Using data from...
Consider the following gas-phase reaction: C2H2(g) + 4 Cl2(g) 2 CCl4(g) + H2(g) Using data from Appendix C of your textbook calculate the temperature, To, at which this reaction will be at equilibrium under standard conditions (Go = 0) and choose whether >Go will increase, decrease, or not change with increasing temperature from the pulldown menu. To = K, and Go will ---Select--- increase decrease not change with increasing temperature. For each of the temperatures listed below calculate Go for...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT