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EQUILIBRIUM REVIEW SHEET 2:
#1) Explain about in what conditions a chemical equilibrium occurs. Explain about what it
means. Explain why limiting reactants does not work in a chemical equilibrium..#2) The following chemical reaction, N2 O 4⇌ 2NO2 + 57.2 kJ, is at equilibrium; however, the
N2O 4 starts with only N-15 isotope and the NO2 is N-14 isotope. At equilibrium, the concentrations will not change. What will happen to the isotopes of nitrogen?
#3) In the above reaction which way would the reaction shift in the following conditions and how would the equilibrium constant change:
a) NO2 is added.
b) N2O 4 is added.
c) A catalyst is added.
d) The system is heated.
e) The total pressure is increased. f) The volume is increased.
g) N2 gas is added.
h) The temperature is decreased.
#4) State five reactions where equilibrium occurs around us. important?
Why is the equilibrium constant
Write the equilibrium constant for #5,6. These are the equilibrium conditions.#5) ____ N2O4 ⇌ ____ NO2 [N2O4] = 0.65 M, [NO2] = 0.25 M
#6) ____ HI + ____ H2O2 ⇌ ____ H2O + ____ I2[HI] = 0.55 M, [H2O2] = 0.80 M, [H2O] = 0.50 M, [I2] = 0.75 M
#11) H O (aq) + SO (g)⇌H SO (aq) K = 1.5 x 103 Initial conditions are [H O ] = 1M, SO (g) 22 2 24 c 22 2
= 0.5M, H2S O4 = zero. What are the equilibrium conditions? Find through the quadratic equation and through approximation.
#12) N2O 4( g) + S8( s) ⇌ SO2( g) +N2( g) The equation is not balanced. If the initial conditions
are [SO2] = 15atm, [N2] =5atm, [N2O 4] =3atm, S8 = 15g. What a re the equilibrium concentrations for the following constants?
a)Kp=1.4×101 2 b)Kp=5.0×10-14 c)Kp=24 IftheKp=1.4×101 0, whatisK?
#13) 2HF(g) ⇌ H2( g) + F2( g). Kp = 16.
following initial conditions?
a) [HF] = 1atm. [H2] =[F2] = 0
b) [HF]= [H2] =[F2] = 1atm
c) [HF]= [H2] =[F2] = 1M
d) [HF] = 1atm. [H2] =[F2] = 0.5atm
e) [HF]=1atm. [H2] =2atm. [F2] =0.5atm
What are the equilibrium concentrations for the
#14) Which types of reactions have a VERY HIGH Kc value? Why?
#15) If A + 2B ⇌ C + D. Kc = 50 E2 + D ⇌ F Kc = 12
E2 + A ⇌G Kc= 40
2A +2B ⇌G Kc= 100
What is the value of the following reaction? 2 C + 2F ⇌ 4E2 A + B⇌0.5G?
Equilibrium Constants of Multiple Reactions Finding #1) At 900 ̊C, Kp =1.04 for the following reaction
CaCO3( s) ⇌CaO(s) + CO2(g).At 900 ̊C, Kp = 0.05 for the following reaction 2FeO(s) + CO2( g) ⇌ Fe2O 3( s) + CO(g)What is the equilibrium constant forCO(g) + Fe2O 3( s) + CaO(s) ⇌ 2FeO(s) + CaCO3( s)
#2) N2( g) + 3H2( g)⇌2NH3( g) has a Kc = 1.3 x 10-2At the same temperature, 2H2( g) + O2( g) ⇌ 2H2O (g), Kc = 3.4 x 103
What is the equilibrium constant for
2NH3( g) + 1.5O2( g) ⇌ 3H2O (g) + N2(g)
#3) N2( g) + 3H2( g) ßà 2NH3(g) has a K = 1.3 x 10- 2At the same temperature, H2( g) + Br2( g) ßà 2HBr (g), K = 3.5 x 104
What is the equilibrium constant for
1.5 Br2( g) + NH3( g) ⇌ 3HBr(g) + 0.5N2( g)
LOOK AT THE FOLLOWING REACTIONS. CAN THEY BE SOLVED EASILY? IF THEY CAN, SOLVE THEM. FIND THE EQUILIBRIUM CONCENTRATIONS.
#23) CaSO4( s) ↔ CaO(s) + SO3( g) K = 10
Start with 10 grams of calcium sulfate, 5 grams of calcium oxide, 2M of SO3.
#24) 8Na2S 2O 3( aq) ↔ 8Na2S O3( aq) + S8( s) K = 10,000 [Na2S 2O 3] = 1M [NaSO3 ] = 1M
#25) 2NO2( g) ↔ N2O 4( g) Kp = 100 [NO2] = 2atm [N2O 4] = 5atm
#26) CH4( g) + 2O2( g) ↔CO2(g) + 2H2 O(l) K = 10,000
[CH4] = 1.5M#27) 8O2 + S8( s) ↔ 8SO2(g)
[O2] = 1M Products = zero. K=256
[SO2( g)] = 0.5M
Al = 100g HCl(aq) = 1.000M Products = zero.
#29) Na2S O4( aq) + 2HCl(g) ↔ NaCl(aq) + 2NaHSO4 ( aq) [Na2S O4] = 1M [HCl] = 1M Products = zero.
#30) H O+ (aq) + OH- (aq) ↔H O(l) K = 101 4 3 2
[H3O +] = 1.5 x 10-8 [OH-] = 1.5 x 10-6#31) NH (g) + H O(l) ↔ NH +(aq) + OH-(aq) K = 1.5 x 10-5
[O2( g)] = 0.5M S8( s) = 100g#28) 2Al(s) + 6HCl(aq) ↔2AlCl3( aq) + 3H2 ( g) K = 10,000
3 2 4[NH3] = 0.05M H2O = 1 liter. [NH4+ ] = 1.5M [OH-] = 1M
#32) OF (g) + H O (g) ↔ 2HF(g) + O (g) K = 1.6 x 106 22 2
Initial conditions, reactants = zero. [HF] = 0.8M [O2] = 1.5M
#8) Lead (II) iodide has a Ksp of 1.4 x 10- 8. If 1g of Pb(II) iodide is put into 1 liter of water, what percent of it will dissolve? (3)
K = 8
#9) 0.5g of NaOH is dissolved in 1 liter of water. 0.5g of Ca(NO3)2 is also dissolved in the same water. Sodium and nitrate ions are completely soluble in water. Ca(OH)2 has a Ksp of 1.3 x 10-6 at 25°C. Will there be a precipitate? Show your work. (3)