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※ 編輯: IboNySun 來自: 140.112.247.72 (10/31 22:24)
課程名稱︰普通化學甲
課程性質︰必帶
課程教師︰陳逸聰教授
開課系所︰化學系
考試時間︰3小時
試題 :
1.In early experiments to charaterize the atom, there are several
simple but very beautiful works. Please briefly describe the
experiments in relation to the determinations of the electron mass,
the electorn charge, and the atomic model. (15%)
2.The material that is made of pure carbon can now be categorized three
types. Could you give these three types and describe the structural
differences among them? (9%)
3.(a)Name the following compunds (5%)
Mg3(PO4)2
Al2(SO4)3
SF6
CuI2
BaCrO4
(b)Write the formula for the following compounds(5%)
sodium sulfite
tin(IV) fluoride
chromium(III) carbonate
diphosphrous pentoxide
chloric acid
4.A salt contains only barium and one of the halide ions. A 0.158g
sample of the salt was dissolved in water, and an excess of sulfuric
acid was added to form barium sulfate(BaSO4), which was filtered,
dried and weighed. Its mass was found to be 0.124g. What is the
formula of the barium halide? (4%)
(Ba=137.3 S=32.07 F=19.00 Cl=35.45 Br=79.90 I=126.9 At=210)
5.Ammonia reacts with O2 to form either NO or NO2 according to
these unbalanced equations:
NH3 + O2 -->NO + H2O
NH3 + O2 -->NO2 + H2O
In a certain experiment 2.00mol of NH3 and 10.00mol of O2 are
contained in a closed flask. After the reaction in complete,
6.75 mol of O2 remains. Calculate tge number of moles of NO in the
product mixture. (Hint: You can't do this problem by adding the
balanced equations, because you can't assume that the two reactions
will occur with equal probability.) (6%)
6.Consider a 1.50g mixture of magnesium nitrate and magnesium chloride.
After dissolving this mixture in water, 0.500M silver nitrate is added
dropwise until precipitate formation is complete. This mass of the white
precipitate formed is 0.641g (Ag=107.9)
(a)Calculate the mass percent of magnesium chloride in the mixture.
(b)Determine the mininum volume of silver nitrate that muse have
been added to ensure complete formation of the precipitate.
7.Please give examples to acid-base reaction, oxidation-reduction
reaction and precipitation reaction.(6%)
8.A compound Z is known to have a composition of 34.38% Ni, 28.13% C,
and 37.48% O. In a experiment 1.00L of gaseous Z is mixed with 1.00L
of argon, where each gas is at P=2.00atm and T=25 degrees centigrade.
When this mixture of gases is put in an effusion chamber, the ratio
of Z molecules to Ar molecules in the effused mixture is 0.4837.
Using these data, calculate the following.
(Ni = 58.69 C=12.011 O=15.999 Ar=39.95)
(a)the empirical formula for Z (4%)
(b)the molar mass for Z (4%)
(c)the molecular formula for Z (3%)
(d)the mole ratio of Z to argon in a sample of gas obtained by
five effuision steps (starting with orginal mixture) (4%)
9.The Maxwell-Boltzmann distribution is given as follows.
f(u)=4*pi*(m/2*pi*k*T)^1.5*u^2*e^(-mu^2/2kT)
u=velocity k=Boltzmann's constant m=mass
(a)Could you get the equation for the most probable velocity Ump,
from the Maxwall-Boltzmann distribution law? (5%)
In an experiment to study the collisions in NH3 molecures, we prepares
the NH3 sample at 600K and 100mTorr.
(b)Could you estimate the number of NH3 molecules in 1cm^3 at this
experimental condition? (5%)
(c)If the radius of the collisional cross-section for NH3 molecules
is 30 angstrom, could you calculate the mean free path for the
NH3 molecules in the sample? (5%)
(d)Using the Ump obtained in question (a) could you estimate the
collisional time period for the NH3 molecules in the sample? (5%)
10. (a)To describe the behavior of real gases, we need to make corrections
to the ideal gas law, PV=nRT. The usual equation to represent
real gases is van der Waals equations. Could you write down the
van der Waals equation and explain the physical meanings of
the correction terms. (7%)
(b)From the following values of van der Waals constants, could
you provide some reasons as to why the constants vary in
such a way? (8%)
a(atm L^2/mol^2) b(L/mol)
He 0.034 0.0237
Cl2 6.47 0.0562
CH4 2.25 0.0428
NH3 4.17 0.0371
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