Reference no: EM131709961

Question 1
Match the following descriptions to the corresponding property notation

Question 2

Choose which of the following are TRUE. Pick ALL answers that are correct

A. The chemical potential it also called the partial molar Gibbs energy of a given species i
B. The chemical potential is also called the Gibbs energy of a pure species i
C. A binary solution of species A and B is in equilibrium with its vapour in a closed system. This means that the binary liquid solution has the Same T and P as its vapour. but the chemical potential of A in the liquid is different to that In the vapour phase.
D. The chemical potential of species i in a mixture is defined as [∂(nG‾)/∂n_i]_T,P,nj
E. The chemical potential of species I in a mixture is defined as [∂(G)/∂n_i]_T,P,nj
F. The chemical potential of species I in a mixture is defined as [∂(nG)/∂n_i]_T,P,nj

Question 3
30.7 cm³ of pure methanol (species 1) and 49.6 cm³ of pure water (species 2) are mooed at room temperature. Mat is the total volume of the resulting solution? Give your answer in cm³ to 1 decimal place.

Given: Partial molar volumes at the given solution concentration are V₁‾ = 38 cm³/mol and V₂‾ =18 cm³/mol. The molar volumes of pure species are 40.727 cm³ mol and 18.068 cm³/mol respectively.

Question 4

Which of the following are TRUE? Choose ALL answers that apply.
A. For a pure species. coexisting liquid and vapour phases at equilibrium have the same T and P. but different fugacities in each phase.
B. For Ideal Gases, the fugacity coefficient is 1. ie, f_i= P.
C. The activity coefficient of a species i is the ratio of its fugacity in a real solution to its fugacity in an ideal solution (at the same T,P and composition)
D. The fugacity of pure species i, f_i is defined in relation to the Gibbs free energy of pure species as follows: G_i = Γ_i(T) + RT Ln f_i
E. The Lewsi/Randall rule applies to each species i in an ideal solution and is given by f^{^id}_i = x_if_i
F. Excess properties are zero for ideal solutions.

Question 5

n-butane C₄H₁₀ (g) undergoes a cracking reaction to form C₂H₄ (g) and C₂H₆ (g) Using the data in Table C4, calculate the standard enthalpy change of reaction at 298 15K, ΔH°₂₉₈. Give your answer to the nearest J.

Question 6

n-butane C₄H₁₀ (g) undergoes a cracking reaction to form C₂H₄(g) and C₂H₆ (g). Using the data in Table C4, calculate the standard Gibbs energy change of reaction at 298 15K ΔG°₂₉₈:, Give your answer to the nearest J.

Question 7

Using your answer to questions 5 and 6 for ΔH°₂₉₈ and ΔG°₂₉₈ calculate the equilibrium constant K at a reaction temperature 742.2 K for the cracking of n-butane C₄H₁₀ → C₂H₄ + C₂H₆. use Cp/R data from table C1 for this calculation and take R = 8.314 j/(mol.K). Give your answer for J to to 2 decimal places.

Question 8

The following reaction reaches equilibrium at 350° C and 2.3 bar, with an equilibrium constant K = 3.7064 at these conditions:

CH₃CHO (g) + H₂(g) → C₂H₅OH(g)

if the system initially contains 1 mol of H₂ and 1 mol of acetaldehyde. what is the extent of reaction? Assume ideal gases. Give your answer to 2 decimal places.

Question 9

The following reaction reaches equilibrium at 350° C and 1 bar, with an equilibrium constant K = 3.7064 at these conditions:

CH₃CHO (g) + H₂(g) → C₂H₅OH(g)

If the system initially contains 1 mol of H₂,1 mol of acetaldehyde and 1 mol of N₂, what is the gas-phase composition of N₂ when the reaction reaches equilibrium? Assume ideal gases and assume N₂ is inert under these conditions. Give your answer to 2 decimal places.

Attachment:- Appendix.pdf