Module A2_ Single Component Systems_ MSE318H1 S LEC0101 20211_Phase Transformations

Why do most polymer blends exhibit lower critical solution temperatures, rather than upper critical solution temperature?   Please describe in relation to entropy and Gibbs free energy. and also i want to know why polymer blends have the behavior of LCST ( compare with UCST )

CO₂ has a positive slope on the melting (fusion) curve. Using the questions below as a guide, show that CO₂ expands upon melting, without employing the Clausius-Clapeyron equation. (i) (ii) (iii) Sketch the specific Gibbs free energies of both phases as a function of pressure using the p - T phase diagram. Use derivatives of the specific Gibbs free energies to obtain the sketch. Sketch the specific volumes of both phases as a function of pressure. Explain how you obtained the sketch of the specific volumes, hence show that CO₂ expands upon melting.

Please solve this questionnnnnn correctly, question please, please UR solution

In the systems given below determine the number of phases, number of components with names and degrees of freedom using the Gibbs Phase rule. I. S(rhombic) ⇆ S(monoclinic) ⇆ S(liquid) ⇆ S(gas) II. PCl5 (g) ⇆ PCl3 (g) + Cl2 (g) i) PPCl3 = PCl2 ii) PPCl3 ≠ PCl2 (PA – is partial pressure of A)

Could you help me with #4? I included a picture of the phase diagram that was given.

REFER TO IMAGE

1/5 For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. Note for advanced students: you may assume ideal gas and ideal solution behaviour. System Change AS O AS 0 not enough information O AS 0 and 34°C. pressure kept constant at 4 atm. not enough O. information O AS 0 dissolved in water. not enough information Enplanation Check Terms of Use | Privacy Center | Accessibilit 02022 McGraw Hill LLC. All Rights Reserved. DE O O O O O

The Gibbs energy of a pure substance is identical to another thermodynamic quantity: the chemical potential, . How does the chemical potential of liquid water relate to the chemical potential of solid ice at standard pressure (1 bar)? How does this change at high pressure? Does the rate at which the wire moves through the ice depend on the amount of weight placed on the wire? If so, how? Consider whether or not this is an equilibrium process. Does it matter how thick the wire is? If so, why? Does it matter if the wire can conduct heat? If so, why?

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. Note for advanced students: you may assume ideal gas and ideal solution behaviour. System Change AS O AS 0 water. not enough information AS 0 14°C. pressure kept constant at 1 atm. not enough information O AS 0 both at 37.°C. flows through the bag into the sucrose solution. not enough O information ?

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. Note for advanced students: you may assume ideal gas and ideal solution behaviour. System Change AS O AS 0 not enough information O AS 0 not enough information O AS 0 pressure kept constant at 3 atm. not enough information

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. Note for advanced students: you may assume ideal gas and ideal solution behaviour.

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. Note for advanced students: you may assume ideal gas and ideal solution behaviour.

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. Note for advanced students: you may assume ideal gas and ideal solution behaviour. System A liter of seawater at 15°C. A 0.35 M solution of sucrose in water, and a beaker of pure water, both at 37. °C. 20. L of pure oxygen (0₂) gas and 20.0 L of pure carbon dioxide (CO₂) gas, both at 5 atm and 22°C. Change The seawater is passed through a reverse-osmosis filter, which separates it into 750. mL of pure water and 250. mL of brine (very salty water). The solution is put into a semipermeable bag immersed in the water, and 50. mL of pure water flows through the bag into the sucrose solution. The gases are mixed, with the pressure kept constant at 5 atm. X AS AS 0 not enough…

4 The Liquid-Vapor Equilibrium line in a one component system should always have a positive slope on a Pressure-Temperature diagram. Explain why? Draw a neat phase diagram of a one component system that can exist in two allotropic forms.

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. Note for advanced students: you may assume ideal gas and ideal solution behaviour. System A liter of seawater at 15° C. 20. L of pure nitrogen (N₂) gas and 20.0 L of pure carbon dioxide (CO₂) gas, both at 3 atm and 37°C. A 0.35 M solution of sucrose in water, and a beaker of pure water, both at 37. °C. Change The seawater is passed through a reverse-osmosis filter, which separates it into 750. mL of pure water and 250. mL of brine (very salty water). The gases are mixed, with the pressure kept constant at 3 atm. The solution is put into a semipermeable bag immersed in the water, and 50. mL of pure water flows through the bag into the sucrose solution. X AS AS 0 not…

In this lab, you will determine the vapour pressure (P) of water at various temperatures and use this data to find its enthalpy of vaporization (AvapH). More generally, for an unknown liquid: if a plot of in P vs. 1/T gives a slope of -5949 K, what is its AvapH in kl/mol? Do not worry about how realistic the value is. Assume R = 8.314 J mol-¹ K-¹ Answer:

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy s of the system, decrease s, or leave s unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. ado Note for advanced students: you may assume ideal gas and ideal solution behaviour. System Change AS O AS 0 at 41 °C. not enough information O As 0 and 2° C. pressure kept constant at 2 atm. not enough information O AS 0 water and 250. mL of brine (very salty water). not enough information O O Olo o

Please help me understand

6. Consider the chemical equation: CO2 + H₂O → C6H12O6 + O2 To balance this equation, place coefficients x, y, z, t in front of each molecule, and for each element, derive a linear equation representing the balance of that element between the two sides. Solve the resulting linear system. How many degrees of freedom (i.e. how many free parameters) are there in your space of solutions? Why does this make sense for the problem we are solving? Choose a particular solution so that all the coefficients are positive integers and write the balanced chemical equation.