Mass of evacuated syringe assembly: 36.9758g Mass of syringe assembly with Dust-Off spray: 37.1017g Mass of Dust-Off spray: 0.1259g Volume of water in syringe: 51mL Volume of Dust-Off spray (should be same as water): 51mL Air temperature: 23.3*C Atmospheric pressure: 729.0 atm Number of moles of Dust-Off spray based on the above P,V, and T: Experimentally determined molar mass of Dust-Off spray:

Mass of evacuated syringe assembly: 36.9758g Mass of syringe assembly with Dust-Off spray: 37.1017g Mass of Dust-Off spray: 0.1259g Volume of water in syringe: 51mL Volume of Dust-Off spray (should be same as water): 51mL Air temperature: 23.3*C Atmospheric pressure: 729.0 atm Number of moles of Dust-Off spray based on the above P,V, and T: Experimentally determined molar mass of Dust-Off spray:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Can you help me with question 1? Thank you!
You find an old, 3-L pressurized bottle of Freon 12 (dichlorodifluoromethane, CCl2F2, MW= 120.91 g/mol) at a dump site with a gauge indicating 2.7 atm of pressure. The temperature is 10° C. How much Freon 12 is still remains in the bottle? The following data are available: Tm = -158.0° C, Tb =-29.8° C). %3D %3D T C) P° (atm) CI -29.8 1 -12.2 16.1 42.4 74.0 5 10 20 CI F
A can of hairspray is 0.34L in volume, at an internal pressure of 3.83atm and at room temp of 25.0C. The can falls into a fire pit and rapidly heat up to 331C and then explodes when the can breaks open. What pressure in atm was enough to break the can open?
A student is performing the airbag experiment, but has three plastic zipper bags available. The volume of each bag is reported below: Sandwich bag: 748 mL Quart bag: 985 mL Gallon bag: 3850 mL The temperature in the room is 21 oC and the pressure is 638 torr. 1 atm = 760 torr and R = 0.08206 L atm/(mol K) In the scenario above, if 6.54 g of sodium hydrogen carbonate is combined with a slight excess of acetic acid solution, how much carbon dioxide, in mL, would be produced? (do not include the units in your answer)
A gallon of octane combusts with O2 (g) to form CO2 and water, according to the balanced equation below: 2C8H18 (1)+ 2502 (g) → 16 CO2(g) + 18 H2O (g) limiting → Assuming excess O2, how many kg of CO2 is released into the air at STP? (Note: 1 gallon = 3.785 L, and octane's density is 0.70 kg/L)
*00 LL L山 A sample of an unknown compound is vaporized at 180. °C. The gas produced has a volume of 2410. mL at a pressure of 1.00 atm, and it weighs 2.08 Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits. OU mol 5. Continue Submit Assignmen O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center | Accessibility MacBook Pro F3 F5 F7 F8 F10 64 $4 # 5. R. B option command command option
In the event of a car crash, a crash sensor sets off a sequence of events that ignites a charge,usually solid pellets of sodium azide (NaN3(s)). The sodium azide explodes and producesenough nitrogen gas to fill a deflated nylon airbag at more than 300 km/h. How many grams of NaN3 ] gs must be included in the canister to produce 67.0 L of nitrogengas at a pressure of 100 kPa and 25.0 °C? What mass of the by-product, sodium metal, is produced in reaction I when the 67.0 L ofnitrogen gas is generated?
Ili Σ 00 %23 %24 96 dp atm inside the bottle? atm and 546.9°C. The bottle is capped, and the dry ice changes to gas. What is the final pressure A piece of dry ice (solid CO,) weighing 11.5 g is placed in a 0.500-L bottle filled with air at 0.968
No Spac. Heading 1 Heading 2 Title Subtitle Paragraph Styles A cylinder in a research laboratory contains 113 kg of chlorine gas at 22.0 °C and 241 atm. The cylinder is equipped with a pressure relief valve that ensures that the maximum pressure does not exceed 500.0 atm. During a fire in the laboratory, the cylinder is exposed to temperatures of 765 °C. (a) What mass (in kilograms) of chlorine is vented (lost)? (b) What is the pressure (in atm) inside the cylinder after the fire is extinguished and the cylinder has cooled to its original temperature? Show all your work, including a complete dimensional analysis.