1) A For NO2, write an equation that shows how the anion acts as a base. Express
ID: 882719 • Letter: 1
Question
1)
A
For NO2, write an equation that shows how the anion acts as a base.
Express your answer as a chemical equation. Identify all of the phases in your answer.
B
For ClO2, write an equation that shows how the anion acts as a base.
Express your answer as a chemical equation. Identify all of the phases in your answer.
2)
A
Write chemical equations for first ionization step of carbonic acid.
Express your answer as a chemical equation. Identify all of the phases in your answer.
B
Write chemical equations for second ionization step of carbonic acid.
Express your answer as a chemical equation. Identify all of the phases in your answer.
3)
Part A
Rank the following compounds in order of decreasing acid strength using periodic trends.
Rank the acids from strongest to weakest. To rank items as equivalent, overlap them.
(H2S, HCl ,HI ,H2O)
Strongest Acid-> Weakest Acid
Part B
Without consulting the table of acid-dissociation constants, match the following acids to the given Ka1values.
Drag the appropriate items to their respective bins.
(H2SO4, H2S, H2SO3)
Ka1= 1.7*10^-7
Ka1= 1.7*10^-2
Ka1= very large
4)
Consider the following reaction:
CO(g)+2H2(g)CH3OH(g)
A reaction mixture in a 5.17 L flask at a certain temperature initially contains 26.5 g CO and 2.36 g H2. At equilibrium, the flask contains 8.67 gCH3OH.
Part A
Calculate the equilibrium constant (Kc) for the reaction at this temperature.
5)
For the following reaction, Kc = 255 at 1000 K.
CO (g) + Cl2 (g) COCl2 (g)
A reaction mixture initially contains a COconcentration of 0.1510 M and a Cl2concentration of 0.178 M at 1000 K.
A
What is the equilibrium concentration of Cl2 at 1000 K?
Express your answer in molarity to three significant figures.
B
What is the equilibrium concentration of COCl2 at 1000 K?
Express your answer in molarity to three significant figures.
6)
For the reaction
2CH4(g)C2H2(g)+3H2(g)
K = 0.150 at 1677 C . What is Kp for the reaction at this temperature?
Express your answer numerically.
Explanation / Answer
1 )
A ) NO2- (aq) + H2O (l) ----------------------> HNO2 (aq) + OH-(aq)
B) ClO2- (aq) + H2O (l) ----------------------> HClO2 (aq) + OH-(aq)
2)
A ) H2CO3 (aq) + H2O (l) -----------------------> HCO3- (aq) + H3O+ (aq)
B ) HCO3- (aq) + H2O (l) -------------------> CO3^-2 (aq) + H3O+ (aq)
3)
3)
Part A
HI > HCl > H2S > H2O
Part B
H2SO4, ------------> Ka1= 1.7*10^-2
H2SO3 --------------->Ka1= 1.7*10^-7
H2S------------------->Ka1= very large
4)
Part A
Calculate the equilibrium constant (Kc) for the reaction at this temperature.
molarity of CO = (26.5/ 28 ) x 1/5.17 = 0.183 M
H2 molarity = (2.36 / 2) x 1/5.17 = 0.228 M
CH3OH molarity = 8.67 / 32 ) x 1/5.17 = 0.0524
CO + 2H2 ----------------> CH3OH
0.183 0.228 0 -------------------> initial
0.183-x 0.228-2x x
but x = 0.0524
[CO] = 0.183-x = 0.13 M
[H2] = 0.228-2x = 0.1232 M
[CH3OH] = x =0.0524 M
equilibrium constant
Kc = [CH3OH] / [CO] [H2]^2
Kc = 0.0524 / 0.13 x (0.1232)^2
Kc = 26.55
5)
For the following reaction, Kc = 255 at 1000 K.
CO (g) + Cl2 (g) COCl2 (g)
A reaction mixture initially contains a COconcentration of 0.1510 M and a Cl2concentration of 0.178 M at 1000 K.
CO (g) + Cl2 (g) <----------------> COCl2 (g)
0.1510 0.178 0 -------------------> initial
0.1510-x 0.178-x x ----------------------> equlibrium
Kc = x / (0.1510-x ) x (0.178-x )
255 = x / (0.1510-x ) x (0.178-x )
by solving this
x = 0.136
A)
equilibrium concentration of Cl2 = 0.178-x = 0.0420 M
B
equilibrium concentration of COCl2 = x = 0.136 M
6)
T= 273 + 1677 = 1950 K
Kc = 0.150
Dn = 2
Kp = Kc (RT)^Dn
Kp = 0.150 (0.0821 x 1950)^2
Kp = 3844.6
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