課程名稱︰普通化學丙 課程性質︰群組必修 課程教師︰蘇志明 開課學院：工學院 生物資源暨農學院 開課系所︰工科系 機械系 生工系 考試日期（年月日）︰2012年3月29日 考試時限（分鐘）：110分鐘 是否需發放獎勵金：是 （如未明確表示，則不予發放） 試題 : 1. Give the full English names for following ionic compounds: (10%) (a) K2SO4 (b) Ba(OH)2 (c) FeCl3 (d) Ni(ClO4)2 (e) NH4Br 2. Give the full English names for the following acids and binary compounds: (10%) (a) HCl (b) H2SO3 (c) Cl2O (d) N2O4 (e) HCO3¯ 3. (a) The electronic state of a hydrogen atom is labeled as (n,l,m,ms). Give the formal names of these four numbers. (5%) (b) Explain the physical implications (or related physical properties) of these four numbers. (5%) (c) With the help of the above labeling of electronic state, explain the working process of the Pauli Exclusion Principle and Hund's rule in building-up the electronic states of atoms. (5%) (d) Consider the wave function of the 1s atomic of H atom. There are two types of probability densities in describing the electron spatial distrubution i.e. probability density and radial probability density. Give the mathematical meaning for these two types of probability densities. Roughly sketch the function behaviors oh these two densities for 1s atomic orbital along the radial axis r. (5%) 4. Consider 1 mole of N2 gas undergoing the change from an inatial state(P1,V1 ,T1) to a final state of (P2,V2,T2), in which P,V and T represent pressure, volume, and temperature, respectively. (a) Assuming that the gas behaves ideally, and we know that P1=1.50atm, T1= 298K, P2=0.5atm, and T2=200K, calculate V1 and V2. (5%) (b) There are always many paths one could take to change the gas from one state to another. Consider the special path as followings: a constant volume path of V1 from the initial (P1,V1) state to an intermediate state (P2,V2), and then taking a constant pressure path from (P2,V1) to the final (P2,V2) state. With the conditions listed in part(a), calculate the total work done and the total heat transferred by the gas for this specific path. (5%) (c) Calculate the internal energy change and the enthalpy change for the complete process form state 1 to state 2. (5%) Additional information: (i) The constant-volume and constant-pressure molar heat capacities of N2(g) are 20.8 and 29.1 Joule/(K mol), respectively. (ii) The gas constant R = 0.0821 L atm K^-1 mol^-1 = 8.31 J K^-1 mol^-1 (iii) 1 L atm = 101.3 J 5. There are two different isotopes of bromine atoms. The mass spetrum of Br2 consists of three peaks: (10%) (a) What is the origin of each peak (i.e. what isotopes does each consist)? Note the atomic number of bromine atom is 35. (b) What is the mass of each isotopes? (c) Determine the average molecular mass of a Br2 molecule. (d) Determine the average atomic mass of a bromine atom. (e) calculate the abundance of the two isotopes. 6. Consider the combustion reaction of the normal butane gas: C4H10(g) + 13/2 O2(g) →4 CO2(g) + 5 H2O(g) With the help of the related thermodynamic data as listed below, aswer the following questions: (a) At 1.00 atm, calculate △H of this reaction at 298K and 1000K, respectively. (5%) (b) Calculate the theoretical maximum temperature that could be reached by igniting a mixture of butane and the air (O2/N2 mole ratio 1/4) under 1 atm constant pressure (i.e. the operation condition of a butane stove used in camping or in a picnic). The initial system temperature is assumed to be 298K. (5%) (c) Instead of the air, if pure oxygen was used in (b), what would be the theoretical maximum temperature one could reach in the butane stove? (5%) Related thermodynamic data: (i) Molar heat capacities at constant pressure (J/mol): O2(g)=29.5 N2(g)=29.1 H2O(l)=75.2 H2O(g)=24.8 CO2(g)=37.3 C4H10(g)=97.5 (ii) Standard enthalpies of formation (KJ/mol) at 298K: CO2(g)=-394 C4H10(g)=-125 H2O(l)=-286 H2O(g)=-242 7. Uing the thermodynamic data listed in problems 4 and 6, calculate the change of the enthalpy, and also the change of the internal energy when one mole of liquid water at 25。C is heated to form a 125。C water vapor at constant 1 atm pressure. (10%) 8. The Coulomb's law can be expressed in the force from F = kQ1Q2/d^2 or in the potential form U = - kQ1Q2/d, in which d is the separation between the charge Q1 and Q2, and k = 9.0 ×10^9 N m^2/C^2. (a) Calculate the electric force on an electron (Q=1.6×10^-19 C) exerted by a single proton if the particles are 0.53 ×10^-10 m apart. (5%) (b) Consider the Rutherford's alpha-particle/gold-foil scattering experiment, and instead assume that he was carrying out a proton-proton scattering experiment with one of the two protons being fixed in a space position (just a thought experiment). We now know that the nuclear strong interaction force comes into play at a nuclear separation of around 1×10^-14 m. Calculate the minimum kinetic energy of the colliding proton Rutherford should use in his experiments in order to probe the "size"of the proton. (5%) --

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