4. (a) Determine the reduced pressure (P,), volume (V,), and temperature (T, ) for a 50 L sample of water at 23 bar and 400 K. For H2O gas, Te = 647.14 K, P. = 220.64 bar, and Vc=55.95 L. (b) Determine the pressure, volume and temperature for a sample of hydrogen which is in a corresponding state with the H2O in part (a). For hydrogen, Te = 32.98 K, Pc = 12.93 bar and mc =64.20 L.

Not for a grade!!!

I need help with part A and B

Chemistry helpppp.

a) From the temperature-pressure data graphed in Part A, visually determine the gas pressure at a temperature of 350 K, including units. (b)From the temperature-pressure data graphed in Part A, determine the equation of the line of best fit. (C) What are the units for the slope of the line of best fit determined in question 2? (D) From the equation of the line of best fit determined in Question 2, algebraically determine the gas pressure at a temperature of 350 K, including units and a unit analysis. Note: I only need su part D solve please

5. Does the pressure-volume relationship follow the ideal gas law PV=nRT (is PV constant at constant n and T) Using the room temperature calculate the number of moles in the pressure/volume experiment when the pressure is 1.00atm in 3.1

10b

we use Pv=nRT. Everything here should be related to H2 (g)    --> Chemical equation1Mg +2 HCl à MgCl2 +H2(g) From video : mass of Mg =.0407 g H2 gas volume = 38.2ml Temperature of room=24.0 +273=297k Total Pressure of the room = 30.01 in mmHg Calculations: find total pressure from barometer and convert it to mmHg, 1 in =2.54 cm and 25.4 mm 30.01 in mmHg x 25.4 mm Hg =762.3 mmHg total pressure of room ​    ​​ 1in mmHg  First step- convert g of Mg to mol of H2 0.0407g Mg x 1mol/24 gx 1molH2 = 0.00169mol                                          1mol Mg Second step: Total pressure of gas = Pressure of H2 + P of water 762.3 = p H2 + 22.4    FROM reference (canvas)=Pressure of water at 24 C= 22.4 mmHg n= 0.00169mol H2 Pressure of H2= 762.3-22.4= 739.854  x 1atm/760= 0.973 atm H2 Volume of H2= 38.2 ml /1000 =0.038L H2 Temp= 297K   anwer this quesions with the information provide: Using PV=nRT, Find R=? (No R averge needed)  à 0.973X0.0382=0.00169XRx 297  0.0372=0.50R Then, Percent error…

Please see question 28, just the top one. I figure in this system the pressure is changing and my answer is the original pressure divided by the final pressure is equal to X.  Do I have this correct?     pv= nRT      N and T and R are constants   thus P1V1 = P2V2.