Stopping to ask for directions
2A ⥢ B + 2C
Which way will the reaction proceed if A is added to the system?
Forward
Write the reaction quotient for the following system:
3Cl2(g) + CS2(g) ⇌ CCl4(g) + S2Cl2 (g)
Q = [S2Cl2][CCl4]/[Cl2]3[CS2]
N2O4(g)⟷2NO2(g)KP= 0.36 (at 100°C)
The reaction above is carried out at the same temperature but the vessel contains only the reactant, PN2O4= 0.0550 atm and none of the product. What are the equilibrium partial pressures for N2O4 and NO2
NO2=0.077
N2O4=0.0165
Given the following reaction: X + 2Y ⇌ Z+W
if K is 4.2 x 10-2, calculate the value for K for:
Z + W ⇌X + 2Y
1/K = 24
Which is the weaker acid?
HF(aq)⇌H+(aq)+ F–(aq) K=6.6x10-4
HNO2(aq)⇌H+(aq)+ NO2–(aq) K=7.2 X 10-4
HF
2A ⥢ B + 2C
Which way will the reaction proceed if some of B is removed?
Forward
NaOH(s)⇌Na+(aq)+OH-(aq) Delta H =-44.4 kJ
K= [Na+][OH-]
The reaction below has a k value of 0.771 at 650oC
H2(g)+CO2(g) ⇌ CO(g) + H2O(g)
If 2.00 moles of both H2 and CO2 are placed in a 4.00L container and allowed to react, what are the equilibrium concentrations of all 4 gasses?
CO and H2O = 0.234 M
H2 and CO2 = 0.266 M
Given the following reaction: X + 2Y ⇌ Z+W
if K is 4.2 x 10-2, calculate the value for K for:
3X + 6Y ⇌ 3Z + 3W
K3= 7.4x10-5
A(aq)+ B(aq)⇌C(aq)+ 2D(aq) K = 4.26 x 106
5.00 moles of A and B were dissolved into a 2.00 L container of water. Which of the following are true when the system reaches equilibrium?
A=B
A>B
B>A
A=B
Which way will the reaction shift if pressure is increased?
N2(g)+3H2(g)⇌2NH3(g)
Forwards
What is the equilibrium constant for the following reaction?
HNO2(aq)+ H2O(l)⇌H3O+(aq)+ NO2-(aq)
[NO2-][H3O+]/[HNO2]
A 5.00L vessel is filled with 1.00 mol H2, 1.00 mol I2 and 2.50 mol of HI Kc = 129 at 500K. Calculate equilibrium concentrations of each reagent.
H2(g)+I2(g) ⇌ 2HI(g)
H2 and I2= 0.068M
HI = 0.764
Given the following reaction: X + 2Y ⇌ Z+W
if K is 4.2 x 10-2, calculate the value for K for:
2Z + 2W ⇌ 2X + 4Y
1/k2= 570
A(aq)+ B(aq)⇌C(aq)+ 2D(aq) K = 4.26 x 106
5.00 moles of A and B were dissolved into a 2.00 L container of water. Which of the following are true when the system reaches equilibrium?
C=D
C>D
D>C
D>C
Which way will the reaction proceed if temperature is decreased?
N2O4(g)⇌2NO2 (g) ΔH =+56kJ
Reverse
Write the reaction quotient
Pb2+(aq)+ 2Cl-(aq)⇌PbCl2(s)
1/[Cl-]2[Pb2+]
Calculate the molar solubility of Ca(OH)2 when it is dissolved in a 0.20 M calcium nitrate, Ca(NO3)2, solution. The Ksp of Ca(OH)2 is 1.3x10-6
Ca(OH)2(s)⇌Ca2+(aq)+ 2OH-(aq)
0.0013M
A + B ⇌ AB K= 4.0
AB + D ⇌ E + A K= 3.0
What is the K value for B + D ⇌ E?
12
A(aq)+ B(aq)⇌C(aq)+ 2D(aq) K = 4.26 x 106
5.00 moles of A and B were dissolved into a 2.00 L container of water. Which of the following are true when the system reaches equilibrium?
A>C
A=C
C>A
C>A
The reaction: Fe3+(aq)+ SCN-(aq)⇌FeSCN2+(aq) is an equilibrium reaction that produces a colored product, at equilibrium the reaction is an orange color. The complex ion FeSCN2+(aq) is a very dark reddish brown,while the reactant Fe3+ is a very pale yellow and SCN- is colorless
Predict the color change when HPO42-(aq) was added and precipitated the Fe3+(aq) ions as Fe2(HPO4)3(s).
pale yellow
Calculate the reaction
Cl2(g)+CS2(g)⇌CCl4(g)+S2Cl2(g)
Cl2= 31.1 atm CS2= 91.2 atm CCl4= 2.12 atm S2Cl2= 10.4 atm
8.04x10-6
The Ksp for CaCO3 6.0x10-9 Calculate the molar solubility when dissolved in water
7.7x10-5M
Reaction A: NiO(s)+H2(g)⇌Ni(s)+ H2O(g) KP= 50
Reaction B: NiO(s)+ CO(g)⇌Ni(s)+ CO2(g)KP= 700
Reaction C: CO2(g)+ H2(g)⇌CO(g)+ H2O(g)KP= ?
Calculate the Kp value for Reaction C at this temperature
0.07
A(aq)+ B(aq)⇌C(aq)+ 2D(aq) K = 4.26 x 106
5.00 moles of A and B were dissolved into a 2.00 L container of water. Which of the following are true when the system reaches equilibrium?
A>D
A=D
D>A
D>A