-) Suppose a 250 mL container is divided into two equal compartments. In the left compartment is argon at 0.50 atm and 0°C. The right compartment contains neon at the same temperature and pressure. Find the Gibbs energy of mixing if both gases can be assumed to be ideal.
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- A mixture of ideal gases consist of the following gases by mole fraction 10% CO2 60% H2O and 30% CO. Determine the Gibbs function of the CO in this mixture when the mixture pressure is 9.00 ATM and it's temperature is 800 Kelvin use data from the tables.Consider two separated gases. The first one consists of 2.0 mol of H2 at a pressure of 2.0 atm and temperature 25 °C, and he second one consists of 4.0 mol of N2 at a pressure of 3.0 atm and temperature of 25 °C. The two gases are mixed keeping the total volume constant. Calculate the Gibbs energy of mixing.4. (1) Write the mathematics expression of Gibbs rules. (2) Using the Gibbs rule to discuss of the freedom F of one component system. (3) Draw and discuss the P-T phase diagram of water system.
- Suppose that for a certain phase transition of a solid AransV = +1.0 cm3 mol-1 is independent of pressure. By how much does the Gibbs energy of transition change when the pressure is increased from 1 bar to 3.0 Mbar?Using a methanol-water mixture as a solvent, a supersaturated solution of sodium chloride and sucrose is made in closed container. The system is let to reach equilibrium woth gas and solid phases. Name the phases and components of the system and define the degree of freedom and its meaning.A mixture of A and B has a liquid-vapor phase diagram as shown in the picture which is not ideal. Assume that 1.5 mol of A and 3.5 mol of B were mixed in an isothermal vessel. Then equilibration was done, and the total vapor pressure was determined to be 50.0 torr. Solve for the number of moles of B that is present in the vapor phase. Choose your answer.a. 1.43 mol b. 1.07 mol c. 1.82 mol d. 2.43 mol
- Consider a container of volume 100 L which is divided by the partition into the two compartments of equal size. In the left compartment, there is nitrogen at 1.0 atm and 25 °C. In the right compartment, there is hydrogen at the same temperature and pressure. Calculate the Gibbs energy of mixing and entropy of mixing and when the partition is removed.Calculate the fugacity (f) of carbon dioxide gas at 75.0 bar and 273 K. The vander Waals constants for carbon dioxide are a = 3.54 L? bar/ moP and b = 0.0427 L/mol.Consider an ideal mixture of two liquids, A and B. The image below shows the mole fraction of component A in the vapour plotted against the mole fraction of component A in the solution. The curve has a slope of 1. Which of the following is necessarily true in such a case? Mole fraction of A in the solution O A. A and Bare present in equimolar quantities in the solution. B. A and B are present in equimolar quantities in the vapour that is in equilibrium with the solution. O C. The vapour pressure of A, pa is equal to the vapour pressure of B, p'B. D. The mole fraction of A in the solution, xA =1 E. The mole fraction of B in the solution, xg = 1 moden au v joue aow
- Consider a system where 2.40 mol of CH3CN(g) are converted into CH3CN(1) at 1.00 atm and 82.0 °C. The normal boiling point of CH3CN is 82.0 °C, and AvapH much less than the volume of CH3CN(g). 29.75 kJ mol-1. Assume the volume of CH3CN(I) is What is the enthalpy change for the process described above? Enter your answer in kilojoules accurate to three significant figures. Do not use scientific/exponential notation. AH= Number kJ. What is the work done during the process described above? w= -7087.0 J w= 798.2 J w= -69.9 J w = 69.9 ) w = 7087.0 J O O O2. Draw a rough phase diagram for a binary system and indicate what phases exist, where they are in equilibrium and how many degrees of freedom exist on each equilibrium line. IConsider the following solutions at 20 °C:I: 0.5 moles trifluoroacetic acid in 1.0 mole of waterII: 0.5 moles trifluoroacetic acid in 1.0 mole of acetonitrileWhich solution would have the greater vapour pressure? Justify your answerfully with calculations