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