Equilibrium
Write the K expressions for the following
CO2(g)+H2(g)<−−>CO(g)+H2O(g)
K= [CO][H2O]/ [CO2][H2]
What can we not add to the equilibrium constant
Pure Solid and Pure Liquid
63Li
What are the strongest forces present between NaCl and water
Ion-dipole
N2 (g) + 3 H2 (g) «--> 2 NH3 (g)
[NH3]2/[N2][H2]3
Write the K expressions
H2O(g)+C(s)↔H2(g)+CO(g)
K= [CO][H2]/[H2O]
What letter do we use to express Reactant Quotient?
Q
What would be the the alpha decay for the nucleotide 201Au
210Au-----> 42 He+ 19777 Ir
Initial concentrations (mol/L)
Experiment [A] [B] Initial rate (mol L-1 s -1)
1 [0.020] [0.010] [0.050]
2 [0.020] [0.020] [0.100]
3 [0.060] [0.020] [0.900]
4 [0.020] [0.040] [0.200]
5 [0.010] [0.020] [0.025 ]
Find the value for the rate constant
k=12500
2SO2(g)+O2(g)⟷2SO3(g)+heat
What happens when more O2 is added?
If you want an Ice pratice problem go to 300-500
For each of the equilibrium expression values below, indicate whether products are going to be favored
A. .0045
B. 5
c. 023
D. 4.5x10-7
B. 5
Name all your strong acids and strong bases. (hahah y'all thought this was finna be easy)
Strong acids
- HCL
- HBR
-HI
-H2SO4
-HNO3
-HClO4
- HClO3
Strong Bases
-LiOH
-NaOH
-KOH
-RbOH
-CsOH
-Ca(OH)2
-Sr(OH)2
-Ba(OH)2
Balance the following equation
239Pu+?⟶24296Cm+10n
Alpha particle (42He)
Calculate the number of moles of nonionic solute in 125g of water if the solution freezes at -1.02. Kf=1.86
.0685 moles
If the equilibrium constant for the following reaction is 1x10-7, determine the final concentration of ICl, if 4.0 moles of I2 and Cl2 were entered initially into an empty 1.0 liter flask.
[ICl]=1.2649x10-3
At 900K the equilibrum constant Kp for the following reaction is .345.
2SO2(g)+O2(g)↔2SO3(g)
At equilibrium, the partial pressure of SO2 is 27.3 atm and that is O2 is 12.4 atm. The partial pressure of SO3 at equilibrium is.
56.465
The equilibrium constant is given for one of reactants below.Determine the value of the missing equilibrium constant.
2HD(g)↔H2(g)+D2(g) K=.28
2H2(g)+2D2(g)↔4HD(g) K=?
12.755
How much time will be required for a sample of H-3 to lose 75% of its radioactivity? The half-life of tritium is 12.26 years
24.53 years
A solution of H2SO4 with a molal concentration of 8.010 m has a density of 1.354 g/mL. What is the molar concentration of this solution?
Molarity will be 6.0739
If 5.0 moles of O2 and 4.0 moles of NO were entered into an empty 1.0 liter flask, calculate the equilibrium constant if the amount of NO2 found at equilibrium was 1.5 moles.
k=.0847
The dissociation of acetic acid, CH3COOH, has an equilibrium constant at 25°C of 1.8 x 10-5. The reaction is
CH3COOH (aq) ↔↔ CH3COO- (aq) + H+ (aq)
If the equilibrium concentration of CH3COOH is 0.46 moles in 0.500 L of
water and that of CH3COO- is 8.1 x 10-3 moles in the same 0.500 L, calculate [H+] for the reaction.
[H+]=1.022x10-3
Consider the following reaction and its equilibrum constant
4CuO(s)+CH4(g)<----->CO2(g)+4Cu(s)+2H2O(g) Kc=1.10
At a certain time the reaction mixture contains concentrations of .22M CH4 , .68M CO2 and1.3 M H2O. Which of the following statements is true concerning the system. (basically which way is the reaction going to occur)
The reaction will shift in the direction of reactants.
Q>K
100.0 grams of an isotope with a half-life of 36.0 hours is present at time zero. How much time will have elapsed when 5.00 grams remains?
155.6 hours
What is the molality of NaCl in an aqueous solution in which the mole fraction of NaCl is 0.100?
6.1659
A mixture consisting initially of 2.00 moles of N2, and 5.00 moles of H2, in a 5.00 L container was heated to 900 K and allowed to reach equilibrium. Determine the equilibrium concentration for 2NH3
N2(g) + 3 H2(g) <---->2 NH3 Kc = 7.6 x 10-6 @ 900 K
[NH3]=1.7435x10-7