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- Initial Pressure = 125 kPa, Initial Volume = 125 mL, Final Pressure = 100. kPa, Final Volume = 100. mL and Final Temperature = 75.0oC. Solve for Initial Temperature. Answer: Unit: Blank 1: Blank 2:Student X decided to perform a science experiment, where she wanted to determine the pressure within the classroom. She took a balloon and inflated it to 1.50 L (at 19oC), and then heated up the balloon to 22oC. The balloon grew to a size of 1.9 L after being heated. When released outside, the pressure in the balloon was 103 kPa. What was the original pressure of the balloon, when still inside? Show all work (Formal method)wo spherical vessels of different sizes contain the same gas and are connected by means of a pipe with a valve. Sphere A has a diameter of 5 foot at the given pressure gauge of 50 kgf/cm2. Sphere B contains the same gas at 20 kgf/cm² gauge. The valve is opened and when the properties have been determined, it is found out that the gauge pressure is 36 kgf/cm2. The temperature at the two vessels before and after opening the valve is maintained at 21.1°C. If the barometric pressure is 750 torr and the gas inside the sphere is oxygen, find the following: 1. The pressure at sphere B in psia. 2.. Temperature at sphere B in F. 3. The pressure of the gas when mixed in psia.
- A app.101edu.co Question 49 of 59 The pressure in Denver, Colorado averages about 632 mm Hg. How many atmospheres is this? STARTING AMOUNT ANSWER RESET ADO FACTOR :( ) 0.98692 1 1000 42.5 760 0.832 105 632 1.01325 x 10 6.24 0.001 101.325 14.70 1.01325 mm Hg kPa psi bar atm Pa torr• Two methanol-water mixtures are contained in separate flasks. The first mixture contains 40 wt% methanol and the second contains 70 wt% methanol. If 300g of the first mixture is combined with 400g of the second, what is the mass fraction of the methanol in the product? O a. 0.119 O b. 0.571 O c. 0.276 О с. O d. 0.765Assume the volume of the filter flask is 250.0mL, you added a total 35mL of solution so the initial volume of gas is (250.0mL - 35.0mL)= 215.0mL. Show how you calculate extra volume of gas forced into the burette because the average temp change is -0.23°C. Show you calculations inlcuding units use Charles law. P and n constant
- A gas whose Cv=1.386 kJ/kg.K and R= 0.485 kJ/Kg.K Determine the MW in kg/kgmol.ALEKS - J X HUc Chapter 5 x G convertc X A www-awn.aleks.com/alekscgi/x/lsl.exe/1o_u-IgNslkr7j8P3jH-IQIHQRDYV_6Ux63SypJXz0Coxvwqgg4JkW174Meq7fCi1Pjl. O GASES Calculating partial pressure in a gas mixture Jacquel. A 7.00 L tank at 19.6 °C is filled with 3.42 g of dinitrogen difluoride gas and 5.08 g of chlorine pentafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: dinitrogen difluoride partial pressure: atm mole fraction: chlorine pentafluoride partial pressure: D atm Total pressure in tank: atm+ |/ 00 %24 D. Two bulbs are connected by a stopcock. The 7.50 L bulb contains nitric oxide (NO) at a pressure of 0.340 bar, and the 2.50 L bulb contains oxygen (O,) at a pressure of 0.510 bar. 02 ON After the stopcock is opened, the gases mix and react to produce nitrogen dioxide (CON) 2 NO(g) + 0,(g) – 2 NO,(g) Considering that the volume remains unchanged during the experiment, how does the total pressure in the bulbs change if the reaction is allowed to go to completion? The total pressure will remain constant. O There is not enough information to determine how the total pressure will change. O The total pressure will decrease. O The total pressure will increase. MacBook Pro ( The %23 %24 7. 4. 5. 3. R %3D K. H. B C. option command MOSISO
- 11. What would be the pHin a sample of pure water at 0.0°C? Kw at this temperature is 1.50 x 1015. А. 6.500 В. 7.00 С. 7.412 D. 7.41 Е. 14.00Complete the ideal gas tables. All answers shall be in 4 decimal places. P (kPa) 125 p (kgm/m³) o (m³/kgm) R (kJ/kgm-K) T (K) GAS MW A 17 295 2.22 0.189 370 GAS MW R (kJ/kgm-K) G (k]/kgm-K) G (k]/kgm-K) k C 28.97 1.4 1.7549 1.4782Two flasks of equal volume are connected by a narrow tube (of negligible volume). Initially, both flasks are at 27°C and contain 0.70 moles of hydrogen gas, the pressure being 50,000 Pa. One of the flasks is then immersed in a hot oil bath at 127°C, while the other is kept at 27°C. Calculate the final pressure of the system, in Pa. Calculate the final number of moles of hydrogen gas in the flask that was immersed in the oil bath. R = 0.08205 L atm mol-¹ K-₁ T(K) = T (°C) + 273.15