Density (MW)P = DRT If you had a substance with a molecular weight of 14 g/mole at 45°C at 4.2 atm, the density be? what would If you had a substance with a density of 50 g/L at 450 Kelvin under 120 atm of pressure, what would the molecular weight be?
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- 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 : __________________________p =0.007y^(2)-0.02y+118 if a persons systolic pressure is 130.67 mm hg, what is their age?A 23-year-old woman with a history of asthma was brought to the emergency department by ambulance. She was extremely short of breath. Her level of consciousness was diminished greatly, and she was only able to respond to questions with nods or one-word responses. She had a weak cough, with nearly inaudible breath sounds. After drawing blood gases, she was placed on supplemental oxygen. Vital signs: heart rate, 160 bpm; blood pressure, 120/84 mm Hg; temperature, 37°C; and respiratory rate, 36/min. Her initial blood gas and total hemoglobin results were as follows: pH = 7.330 pCO2 = 25 mm Hg pO2 = 58 mm Hg HCO3 = 13 mmol/L tHb = 12.4 g/L QUESTIONS: 4. What clinical findings are most indicative of this patient’s impending failure?
- the atmospheric pressure in inches Hg (inHg) 30.08 Temperature at beginning of measurements (°C) 20.6 Mass added Syringe volume Reading 1 0.0 5.0 Reading 2 0.300 4.5 Reading 3 0.450 4.2 Reading 4 0.650 4.1 Reading 5 0.950 3.6 Reading 6 1.150 3.1 Reading 7 0.200 5.4 Reading 8 0.400 6.7 Reading 9 0.550 7.5 Reading 10 0.700 8.4 Reading 11 0.900 9.3 Temperature at end of measurements (°C) 20.6 PV Measurements and Calculations Volsyringe (mL) VolT (mL) Mass added (kg) Force (kg·m/s2) Psyr (Pa) PT (Pa) PV (Pa·mL) No mass addedReading 1 5.0 0.000 Increasing the pressureReading 2 4.5 0.300 Reading 3 4.2 0.450 Reading 4 4.1 0.650 Reading 5 3.6 0.950 Reading 6 3.1 1.150 Decreasing the pressureReading 7…A volumetric flask made of Pyrex is calibrated at 20.0°C. It is filled to the 220-mL mark with 42.0°C Mercury. After the flask is filled, the Mercury cools and the flask warms so that the combination of Mercury and flask reaches a uniform temperature of 32.0°C. The combination is then cooled back to 20.0°C. (The average volume expansion coefficient of Mercury is 1.82 10-4(°C)−1.) a. What is the volume of the Mercury when it cools to 20.0°C? b. At the temperature of 32.0°C, does the level of Mercury lie above or below the 220-mL mark on the flask? Explain.Using your cars miles per gallon and the miles you drive in 1 week calculate the liters of carbon dioxide you produce when using your car. Compare your miles in February (pre-covid) versus June (post-covid). Assume that your engine combusts at 1.00 atm and 25.0 celsius. Assume that your gasoline is 100% octane (C8H18). You will also need to balance the combustion reaction that occurs in your car engine. You will need to use PV=nRT I think calculations are not correct specially for June. please help 2C8H18+ 25O2→16CO2+18H2O Feb, (pre covid), Miles covered per week=15×7=105 miles So fuel consumed per week=105 miles/30 miles ga =3.5 ga Density of octane=3.18 kg/ga Mass=volume × density Mass of Octane used per week = 3.5 ga x 3.18 kg/ga =11.13 kg Moles of octane in 11.13 kg 11.13 kg/114 kg/k mol =0.097 kmol 2 kmol octan≡16 kmol CO2 0.097 kmol octane =16/2 × 0.097 kmol CO2 0.097 kmol octane = 0.781 kmol CO2 n= 0.781 kmol=781 moles CO2 V=781 mol x 8.314j/k. mol x (25+273)K/1atm x…
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- A student performed the experiment described in this module, using 4.00 mL of a 3.5% H2O2 solution with a density of 1.61 g mL-1. The water temperature was 25 ° C, and the barometric pressure in the laboratory was 30.40 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 79.20 mL of O2. (8) Calculate the number of moles of H2O2 reacting.What is the kinetic energy of one mole of mercury that has a speed of 200 m/s? (M(Hg) = 0.201kg.mol-1)Solid sodium reacts with liquid water to form hydrogen gas according to the equation 2 Na(s) + 2 H₂O(l) → 2 NaOH(aq) + H₂(g) What is the pressure of hydrogen gas in the 20.0 L headspace of a reactor vessel when 1.82 kg sodium is reacted with excess water at 50.0°C? -don't prematurely round