CH.35/CH. 36
For the process: CCl4(l) → CCl4(g) ; Δ H = 43.0 x 10^3 J. Calculate the ΔS(surr) at 25degreesC.
-144 J/K
For the reaction: N2(g) + 3H2(g) → 2NH3(g) ; ΔH = -91.8 kJ and ΔS = -197 J/K at 25degreesC Calculate ΔG
-33.1 kJ
The system: A(g) ↔ 2B(g) Kc = 1.0 x 10^-4 initially [A] = 0.22M . The equilibrium concentration of B is
0.00469
For: CO(g) + 2H2(g) ↔ CH3OH(g), at equilibrium [CO] = 0.22 ; [CH3OH] = 0.11 ; Kc = 1.2 x 103, what is [H2] ?
0.020
3O2(g) ↔ 2O3(g) ; if 10.0g of O2 is at equilibrium with 7.50g of O3 calculate Kp if the total pressure is 0.110atm.
0.295
For: N2(g) + O2(g) ↔ 2NO(g) 0.500M O2 and 0.750M N2 is allowed to reach equilibrium. Kc = 1.00 x 10^-1. Calculate equilibrium concentration of O2
0.417
For: 4NO2(g) + O2(g) ↔ 2N2O5(g), at equilibrium [NO2] = 0.031 ; [O2] = 0.11 ; [N2O5] = 120 ; the Kc value is:
1.4 x 10^11
For the system: 2NH3(g) + CO2(g) ↔ NH2CONH2(aq) + H2O(l) ; ΔG = -13.6 kJ at 25 degrees Celsius. Calculate the equilibrium constant. (be careful of the negative sign)
2.4 x 10^2
For the system: I2(g) + Cl2(g) ↔ 2ICl(g) at equilibrium 0.310 moles of I2, 0.310 moles of Cl2 and 2.81 moles of ICl was found in a 1L vessel. 1 mole of ICl was then added to the vessel. Calculate the final equilibrium concentration of ICl
3.63
Calculate Keq for the reaction: A(g) + B(g) ⇔C(g) + D(g) given Kp = 3.9 x 10^-6@ 65°C
3.9 x 10^-6
If the reaction quotient is infinity, there are just reactants present and the system will form products to reach equilibrium
False
The system: A + B ↔ 2C ; initially started with 2 moles of B and 1 mol A in a 1L flask. Keq = 4.9 x 10^5 To calculate the equilibrium concentrations a simplifying assumption (approximation) can be made.
False
The third law of thermodynamics states that a perfect crystal at 298K has zero absolute entropy.
False
When the reaction quotient, Q , has a value equal to the equilibrium constant the reaction
Is at equilibrium
For the reaction A(g) + 2B(g) ↔ C(g) ; Kc = 10 Which direction will it proceed if [A] = 0.100, [B]= 0.100 , and [C] = 0.100 is found before equilibrium is established?
Left
For the system: 2CO(g) + O2(g) ↔ 2CO2(g) ; adding CO2 shifts the equilibrium:
Left
For the system: 2CO(g) + O2(g) ↔ 2CO2(g) ; decreasing the pressure will shift the equilibrium:
Left
For the system: 2NO2(g) ↔ N2O4(g) ΔH = -14 kcal ; increasing the temperature will shift the equilibrium:
Left
The process of heating a gas, the entropy change is:
Positive
A process will be spontaneous if ΔG is negative
True
At equilibrium, the concentrations of the products and reactants may not be equal.
True
For the reaction: H2(g) + I2(g) ↔ 2HI(g) The initial equilibrium concentrations are [I2] = 2.11 , [H2] =2.11 and [HI] = 0.299. 1.0M HI is added, the new equlibrium concentration of [H2] will be greater than its initial equlibrium concentration.
True
For the reaction: I2(g) + Cl2g) ↔ 2ICl(g) the Kp value is 3.4 x 10^-2 The Kp value for: 2ICl(g) ↔I2(g) + Cl2g) is 29
True
For the system: 2NO2(g) ↔ N2O4(g) the initial concentration of NO2 was 0.055M. An approximation was made and the equillibrium concentrations were calculated. The unknown "x" in the calculation was found to be 0.0011. The approximation is valid.
True
For: 2COF2(g) ↔ CO2(g) + CF4(g) the Kc value is 2.0 x 10^-4 For: 4COF2(g) ↔ 2CO2(g) + 2CF4(g) the Kc value is 4.0 x10^-8
True
Given: 2X ↔ Y Kc = 0.60 ; Y ↔ Z Kc = 1.1 The Kc value for 2X ↔ Z is 0.66
True
The system: 2CO(g) + O2(g) ↔ 2CO2(g) Kc = 1.0 x 10^5 , initial concentration of CO2 is 0.55M. To calculate the equilibrium concentrations an approximation can be made
True
When a stress is applied to a system at equilibrium, the position of the equilibriun will shift and the equilibrium concentrations may change
True
For the system: 2A ↔ C + B ; the equilibrium constant expression is:
[C][B]/[A]^2
For the system: A + B ↔ C + D ; keq = 4.9 x 10^1 . The equilibrium mixture exist as:
approximately 50% reactants and 50% products
The system: 2NO2(g) ↔ N2O4(g) ΔH = -14 kcal ; increasing the temperature will _____ the equilibriun constant value
decrease
Kc for a system is 16. The equilibrium lies:
in middle
When there is more reactant than product at equilibrium, the equilibrium lies:
left
For the system: 2CO2(g) ↔ 2CO(g) + O2(g) when adding a catalyst, the equilibrium will:
not change