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Calculate the entropy of activation for a collision between two structureless particles at 450 K, taking M = 92 g mol−1 and σ = 0.45 nm2.
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- Derive an expression for the temperature dependence of Kc for a general gas-phase reaction.For how long on average would a hydrogen atom remain on a surface at 400 K if its desorption activation energy is (i) 15 kJ mol−1, (ii) 150 kJ mol−1? Take τ0 = 0.10 ps. Repeat both calculations at 1000 K.Nitrogen gas adsorbed on a surface to the extent of 1.242 cm3 g−1 at 350 kPa and 180 K, but at 240 K the same amount of adsorption was achieved only when the pressure was increased to 1.02 MPa. What is the enthalpy of adsorption of nitrogen on the surface?
- Estimate the change in the Gibbs energy of 100 cm3 of water when the pressure acting on it is increased from 100 kPa to 500 kPa. Given that the mass density of water is 0.997 g cm−3, determine the change in the molar Gibbs energy.Calculate the standard molar entropy of N2(g) at 298 K from its rotational constant ᷉ B = 1.9987 cm−1 and its vibrational wavenumber ᷉v = 2358 cm−1. The thermochemical value is 192.1 J K−1 mol−1. What does this suggest about the solid at T = 0?Discuss the equation for the partition coefficient and the implications of the different values for K (K = 1, K < 1, and K > 1). What does this tell you about the solute?
- Calculate the change in the molar Gibbs energy of a perfect gas when its pressure is increased isothermally from 50.0 kPa to 100.0 kPa at 500 K.Calculate the standard molar entropy of N2(g) at 298 K from its rotational constant B =1.9987cm−1 and its vibrational wavenumber =2358cm−1. The thermochemical value is 192.1 J K−1 mol−1. What does this suggest about the solid at T = 0? PLEASE ANSWER ALL OF THE QUESTION, NOT THE FIRST PART!Is the expansion coefficient a path-dependent parameter? Explain in detail in terms of physical chemistry and also help me with some references regarding this topic.
- Estimate the change in the Gibbs energy of 1.0 dm3 of liquid octane when the pressure acting on it is increased from 1.0 atm to 100 atm. Given that the mass density of octane is 0.703 g cm−3, determine the change in the molar Gibbs energy.The pseudofirst-order rate constant for the decomposition of urea, CO(NH2)(aq) + 2 H2O(I)→ 2 NH4+(aq) + CO32-(aq). is 1.2 x 10-7 s- 1 at 60 °C and 4.6 x 10-7 s-1 at 70 oc. Estimate (a) the activation Gibbs energy and (b) the entropy of activa tion of the reaction.Suppose a compound could point in any of three directions in the solid and still have the same energy. What would be the total entropy (J/K) of orientation if 1.2703e+14 molecules are randomly distributed?