Practice final exam
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Substance A decomposes by a first-order reaction. Starting initially with [A] = 2.00 M, after 126 min [A] = 0.250 M. For this reaction, what is (a) t1/2 ; (b) k ?
T
he
initial rate of the reaction A + B C + D is determined
for different initial conditions, with the results listed in the
following table.
Expt [A],M [B],M Initial rate ( Ms-1)
1 0.185 0.133 3.35 x 10 -4
2 0.185 0.266 1.35 x 10 -3
3 0.370 0.133 6.75 x 10 -4
4 0.370 0.266 2.70 x 10 -3
What is the order of the reaction with respect to A and B ?
What is the overall reaction order ?
What is the value of the rate constant, k ?
W
hen
1.00 mol I2(g)
is introduced into an evacuated 1.00- L flask at 1200 oC,
5% of the I2
molecules dissociate into iodine atoms. For the reaction I2(g)
2I(g) at 1200 oC
What are the values of (a)
Kc
and (b)
Kp
?
Equilibrium is established at 1000 K, where Kc = 281 for the reaction
2
SO2(g)
+ O2(g)
2SO3(g).
The equilibrium amount of O2(g)
in 0.185-L flask is 0.00247 mol. What is the ratio of [SO2]
to [SO3]
in the equilibrium mixture?
What is the (a) degree of ionization and (b) percent ionization of propionic acid in a solution that is 0.45 M HC3H5O2 ?
H
C3H5O2
+ H2O
H3O+
+ C3H5O2-
pKa
= 4.89
6. Calculate the pH at the points in the titration of 25.0 mL of 0.132 M HNO2 when (a) 10.0
mL and (b) 20.0 mL of 0.116 M NaOH have been added. For HNO2, Ka = 7.2 x 10-4.
H
NO2
+ OH-
H2O
+ NO2-
7. Use VSEPR theory to predict the geometric shapes of the following molecules and
ions; (a) N2 , (b) HCN , (c) NO3-, (d) NSF.
8 Nicotine extracted from tobacco leaves, is a liquid completely miscible with water at
temperature below 60 oC. (a) What is the molality of nicotine in an aqueous solution that
starts to freeze at – 0.450 oC? (b) If this solution is obtained by dissolving 1.921 g of
nicotine in 48.92 g H2O, what must be the molar mass of nicotine? (Kf = 1.86 oC/m)
9. Tungsten(W) has a body-centered cubic crystal structure. Using a metallic radius of 139
pm for the W atom, calculate the density of tungsten.
10. The following first-order reaction occurs in CCl4 (l) at 45 oC.:
N
2O5
N2O4
+ ½ O2
(g). The rate constant is k
=
6.2 x 10-4
s-1.
An 80 g sample
of N2O5 in CCl4(l) is allowed to decompose at 45 oC.
How long does it take for the quantity of N2O5 to be reduced to 2.5 g ?
How many liters of O2, measured at 745 mmHg and 45 oC, are produced up to this point.
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