5) Starting from the expression G, – Cy = T (O"/aT), (®V/at), ' use the appropriate relations between partial derivatives to show that T(W/ər), (V/ar), d. Cp – Cy =
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- 6) Calculate the final temperature of a sample of carbon dioxide of mass 16.0 g that is expanded reversibly and adiabatically from 500 cm³ at 298.15 K to 2.00 dm³.(2) The Gibbs function G is (GF) ₁ P == ound ·S (06), = relationship (25) a = -(=++) ₂ thu modynamic property. If =V, prove the followingby plotting appropriate quantities based on equation 6a. determine the values of k' and y.
- The term "bond energy" and "bond enthalpy" have often been used interchangeably to describe the strength of a bond. a) Calculate the average bond enthalpy of the O-H bond in water at 298 K and 1 bar, given the reaction: H₂O(g) →2H(g) + O(g), with AHƒ = 218.0, 249.2, and -241.8 kJ mol¹¹ for H(g), O(g), and H₂O(g) respectively. Give your answer in units of kJ/mol. b) How does your answer from (a) compare to the average bond energy (i.e. AU) of the O-H bond at 298 K and 1 bar: 461.0 kJ/mol?A7. (a) Given that for an ideal gas (0) AG=nRT In aG ap =V, show that for a change in pressure from P₁ to P₂ ompression of twoDescribe how to find the relationshipbetween the state properties (P, V, T ) of agas and its molar mass or density.
- Given the following data: CO(g)+H20(g)→ CO,(g)+ H2(g) AH° (25°C) = -42.0 kJmol1 C, (CO) = 26.8 + 6 x 10³T JK'mol1 C, (H2O) = 30.1+ 10 x 10³T JK'mol1 Cp (H2) = 28.5 + 2 x 10³T JK'mol1 C, (CO2) = 26.4 + 42 x 10³T JK-'mol1 where T is the thermodynamic temperature, calculate the change in enthalpy for the reaction at 1000 K.P2C.4 From the following data, determine A,H° for diborane, B,H,(g), at 298 K: (1) B,H,(g) + 30,(g) → B,O,(s) +3 H,O(g) A̟H° =-1941kJ mol -> %3D (2) 2B(s) + 를0,(g) → B,O, (s) A̟H® =-2368 kJ mol (3) H,(g)+±O,(g) → H,O(g) A,H° =-241.8kJ mol %3DThe table below contains some mean bond energy data: Bond C-C 348 H-H N=N Mean bond energy /kJ mol| 436 944 (i) Balance the equation below for the formation of one mole of ammonia, NH3, from its elements. N2 + H2 NH3 AH = -38 kJmol" (ii)Use the data in the table above to calculate the bond energy of N - H bond in NH3 in the reaction given in (1) above. Comment on why the value obtained is referred to as 'mean bond enthalpy (ii) Use the equation below and data from the table to calculate a value for the C=C bond energy in ethene. Bond H-H C-H C-C 348 Mean bond energy /kJ mol 436 418 нн нн С—С + Н Нэнс- с н AH = -136 kJ mol нн н Ethene Ethane
- Since we will be dealing with partial derivatives later in the semester, this is a good opportunity to review this topic (see appendix C). Then evaluate the following partial derivatives (a) PV = nRT; (∂ P/∂V)T (b) r = (x2 + y2 + z 2 )1/2; (∂ r/∂y)x,zRank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on. substance A B с D H :0: H | || | H с C -C-H 174 H H H chemical symbol, chemical formula or Lewis structure H H H | | C I 1 I H H H (II | Ag - Ar - :O: -O-H boiling point (Choose one) (Choose one) ✓ (Choose one) (Choose one) ✓(ii) Given that ан (он), =C, au - (24) = C₁ Show that Cp - Cy =nRT for n moles of an ideal gas and that