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- Room temperature: 294.0 K Barometric pressure: 770.5 mmHg Vapor of water: 18.6 mmHg Volume of O2 collected: 57.90 mL Density of H2O2: 1.01 g/mL % Composition H2O2: 3.02 % Volume of H2O2 used: 5.00 mL Letter of the unknown solution of H2O2: B Volume of O2 collected for the unknown: 20.20 mL corrected barometric pressure. 752 mmHg Expert, what is a term letter?Calculate the mass, in gg, of 13801380 mLmL of \ce{CH4}CHX4 at STP. show work.Room temperature: 295.9 K Barometric pressure: 769.0 mmHg Vapor of water: 21.1 mmHg Volume of O2 collected: 59.20 mL Density of H2O2: 1.01 g/mL % Composition H2O2: 3.02 % Volume of H2O2 used: 5.00 mL Letter of the unknown solution of H2O2: C Volume of O2 collected for the unknown: 64.90 mL Calculate R in the ideal gas law.
- A syringe with friction free plunger has a pressure of one atmosphere acting down on plunger, 47 C, 1.60 x 10-3 mole, 40.0 mL. if add 1/4 more molecules while temperature is constant, what are the new T, P, and V?A SCUBA driver is 100 ft below the surface of the ocean where the water exerts a pressure 43.3 psi at 18.0o The diver exhales and many bubbles are released and these bubbles rise to the surface where the atmospheric pressure is 1.03 psi and the temperature is 36.0o C. One bubble has a volume of 20.0 mL. What is the volume of the bubble at the surface? You may assume the composition of the bubble does not change and the bubble remains intact as it rises. P1 = P2 = V1 = V2 = n1 = n2 = T1 = T2 =Consider Figure 13.1. If the height of the mercury column in the leveling bulb is 21 mm greater than that in the gas buret and atmospheric pressure is 600 mm , what is the pressure on the gas trapped in the buret? Should I assume (1 atm) or would I assume the atm is 600mm (standard) and subtract the 21 from the 600, then convert by division (600-21)/760 ?? thanks
- An old gas cylinder you found lost its label. Lab supervisor is pretty sure that it is either He, Ne, Ar or Kr and you were tasked to figure out which one. What you did was that you transferred some of the gas from the old cylinder into an evacuated 10-L flask until the gauge pressure inside reached 1.00 atm. After sealing it, you carefully weighed the gas-filled flask and figured out that the mass of the gas (excluding that of the flask) was 15 g. If the temperature and barometric pressure in the lab was 27°C and 1 atm, what was the gas?Room temperature: 294.0 K Barometric pressure: 770.5 mmHg Vapor of water: 18.6 mmHg Volume of O2 collected: 57.90 mL Density of H2O2: 1.01 g/mL % Composition H2O2: 3.02 % Volume of H2O2 used: 5.00 mL Letter of the unknown solution of H2O2: B Volume of O2 collected for the unknown: 20.20 mL Calculate the corrected barometric pressure. 752 mmHg I think the o2 pressure is 733.4 Calculate the volume of O2 at STP in mLA plastic bag is weighed and then filled successively with two gases, X and Y. The following data are gathered: Temperature: 0.0°C (273 K) Pressure: 1.00 atmosphere Mass of empty bag: 20.77 g Mass of bag filled with gas X: 24.97 g Mass of 1.12 liters of air at conditions given: 1.30 g Volume of bag: 1.12 liter Molar volume at STP: 22.4 liters Reference: Ref 5-6 The mass of 1.12 liters of gas Y is found to be 6.23 g. The density of gas Y is Select one: a. 10.6 g/L b. 5.56 g/L c. 15.6 g/L d. 0.200 g/L e. 0.180 g/L
- Dioxins are known to be very toxic. If TCDD concentration in the atmosphere is 195 ng/L of air. What will be the concentration in part per trillion (ppt).A core sample is saturated with an oil (?o = 35oAPI), gas and water. The initial weight of the sample is 224.14 g. After the gas is displaced by water (?w = 1 g/cm3 ), the weight is increased to 225.90 g. The sample is the placed in a Soxhlet distillation apparatus, and 4.4 cm3 water is extracted. After drying the core sample, the weight is now 209.75 g. The sample bulk volume, 95 cm3 is measured in a mercury pycnometer. Find the porosity, water saturation, oil saturation, gas saturation and lithology of the core sample.1) Mass of flask, aluminum foil, and rubber band 68.45g 2) Temp. Of boiling, water 98.20 0C 3) Barometric pressure 755 mmHg 4) Volume of flask (volume of vapor occupies flask) 152 ml 5) Mass of flask, aluminum foil, rubber band, and condensed vapor 68.60g 6) Mass of condensed vapor is (5)-(1) Find Molecular weight of unknown ______ g / mol Calculation PV = (m/M)RT) è M = (mRT) / PV = ? Unknown liquid- Based on Molecular weight determine which unknown below has this molecular weight: Methanol, Ethanol, Isopropanol, Propanol. UNKNOW IS : __________________________