In a 20 ml syringe, covid-19 vaccine is taken at 27°C at a pressure of 104 kPa. The volume of vaccine is expanded to 35 mL by keeping the temperature 40°C during mid-day time. (i) Convert all thermodynamic variable in its Sl unit. (ii) Calculate the pressure in Pascal when the volume is increased.
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- Can you help me show the process in this problem? Thermodnamics At 25 °C 1 mol of an ideal gas is expanded isothermally from 2 to 20 dm3. Calculate ΔA and ΔG. Do the values depend on whether the process is reversible or irreversible? Ans: -5.71 kJ/mol and 5.71 kJ/mole respectively.P:33)In an isochoric process, one mole of an ideal gas of rigid diatomic molecules at volume V is taken from an initial temperature T to a final temperature 4T. Using the convention that heat is positive when it is absorbed by the system, what is the heat transfer in terms of R and T?
- 2.0 moles of an ideal gas is initially at P = 1.0 atm and T = 300 K. It is then taken through a three-step reversible process: (i) isobaric expansion to twice its original volume; (ii) isothermal compression, returning to its original volume; (iii) isochoric reduction in pressure to the original state. Find the work done on the gas in each step of the process and the net work done on the gas for the process.One mole of an ideal gas, in the initial state T=300K, P=10atm, is contained in a piston and is subjected to each following process. (R=8.314 J/mol-K or 0.082 atm-L/mol-K) (1) The gas is irreversibly expanded at an adiabatic condition until its pressure becomes 1 atm. Calculate the final temperature. (external pressure = 1 atm) (2) The gas performs 753.12J of work while it undergoes an adiabatic expansion. Calculate the final temperature. (3) The gas absorbs 50J of heat and performs 100J of work. Calculate the final temperature. (4) 8314J of heat is absorbed during a reversible isothermal expansion. What is the final volume of gas?- (5) The pressure of gas decreases to 1 atm at a constant volume condition. Calculate the change in entropy.eCombustion products in a gas turbine expand adiabatically from a pressure of 4 bar and a temperature of 880ºC to a pressure of 1 bar and a temperature of 550ºC. Assuming the reversible path 1-b-2 and that the process 1-b is adiabatic, determine the ∆s. Consider the value of Cp = 1 J / g K
- One mole of an ideal gas, for which CV,m = 3/2R, initially at 298 K and 1.00 × 10^5 Pa undergoes a reversible adiabatic compression. At the end of the process, the pressure is 1.00 × 10^6 Pa. Calculate the final temperature of the gas. Calculate q, w, ΔU, and ΔH for this process.A cylinder with a piston contains 0.150 mol ofnitrogen at 1.80 * 105 Pa and 300 K. The nitrogen may be treated as anideal gas. The gas is first compressed isobarically to half its originalvolume. It then expands adiabatically back to its original volume, andfinally, it is heated isochorically to its original pressure. (a) Show theseries of processes in a pV-diagram. (b) Compute the temperatures atthe beginning and end of the adiabatic expansion. (c) Compute theminimum pressure. Use the conditions and processes of the problem above tocompute (a) the work done by the gas, the heat added to it, and its internal energy change during the initial compression; (b) the work done by the gas, the heat added to it, and its internal energy change during the adiabatic expansion; (c) the work done, the heat added, and the internal energy change during the final heating.