A sample of a gas at room temperature occupies a volume of 40.0 L at a pressure of 612 torr if the pressure changes to 3060 torr, with no change in the temperature or moles of gas, what is the new volume. V₂? Express your answer with the appropriate units. View Available Hint(s) V₂ = Value Submit Part B μA B If the volume of the original sample in Part A (P-612 torr. V₁ 40.0 L) changes to 57 0 L, without a change in the temperature or moles of gas molecules, what is the new pressure. P Express your answer with the appropriate units. View Available Hint(s) A Units Value Units ?

A sample of a gas at room temperature occupies a volume of 40.0 L at a pressure of 612 torr if the pressure changes to 3060 torr, with no change in the temperature or moles of gas, what is the new volume. V₂? Express your answer with the appropriate units. View Available Hint(s) V₂ = Value Submit Part B μA B If the volume of the original sample in Part A (P-612 torr. V₁ 40.0 L) changes to 57 0 L, without a change in the temperature or moles of gas molecules, what is the new pressure. P Express your answer with the appropriate units. View Available Hint(s) A Units Value Units ?

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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Three gases, A, B, and C, are mixed into one container with a total pressure of 702.1 mmHg. The partial pressure of gas A is 103.8 mmHg. The partial pressure of gas B is 351.0 mmHg. What is the partial pressure of gas C in the container in mmHg? Watch your units and round your answer to the tenths place.
(2)Determine partial pressure
ld=15556158&HeplD=6b9f9b2f... 2 012 ourses Gay-Lussac's law states that the pressure of a gas is directly related to its absolute temperature, provided the volume and number of moles of the gas remain the same: (Figure 1) Review I Constants I Periodic Table Part B Using the same sample of gas (Pi = 615 torr, Ti 37 °C), we wish to change the pressure to 6150 torr with no accompanying change in volume or amount of gas. What temperature T2, in Celsius, is needed to reach this pressure? - P2 T2 Express your answer with the appropriate units. Figure View Available Hint(s) 1 of 1 HA °C T2 0.27 Subm Previous Answers Incorrect; Try Again; 3 attempts remaining Higher temperature Higher pressure Lower temperature Lower pressure Next> Provide Feedback P Pearson Copyright O 2019 Pearson Education Inc. All rights reserved.| Terms of Use Privacy Policy | Permissions | Contact Us 2
I Need answer question 2 using question 1 information QUESTION 1: using the formula for the ideal gas law and the value for the gas constant of 0.08206 L.atm/k/mol, what is the volume (in L) of 7.96 grams of dry hydrogen at 28.3C and 766 torr ( i got this answer as 96.91 L) 、 QUESTION 2: the student obtains the following data by following an experimental procedure to this on. base on this data, what is the value of R in (L.ATM/MOLE/K) that would be calculated? report the result to fours sig fig (using 273.15k for temperature conversion) Pressure of dry h2 = 740.9, temperature = 23.0 degrees C, mass pf mg used =0.037, volume of H2 = 39.45 ET units, conversion factor=1.000 what is the value of R in (L.ATM/MOLE/K) that would be calculated?
A sample of xenon gas occupies a volume of 8.88 L at 47.0°C and 0.920 atm. If it is desired to decrease the volume of the gas sample to 7.50 L, while decreasing its pressure to 0.693atm, the temperature of the gas sample at the new volume and pressure must be ______°C.
A sample of nitrogen gas at 13°C and 760. mmHg has a volume of 8.83 mL. What is the volume of gas at -9°C and 1 atm of pressure? Volume = mL
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Please don't provide handwritten solution ....
A common laboratory system to study Boyle’s law uses a gas trapped in a syringe. The pressure in the system is changed by adding or removing identical weights on the plunger. The original gas volume is 34 mL when two weights are present. Predict the new gas volume when four more weights are added.
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A sample of gas originally at 29.2°C and 1.847 atm pressure in a 5.53 L container is allowed to expand until the pressure is 0.357 atm and the temperature is 23.6°C. The final volume of the gas is L. Record your answer with 3 significant figures.
Two gas tanks contain different gases. The pressure, volume, and termperature of each gas are shown in the diagram. Ne(g) Tank X Tank Y P 120 atm V = 50 L P = 150 atm V = 50 L T 25°C T 25°C Which of the following could explain the difference in the observed pressures? (Assume that the gases behave ideally.) Nitrogen gas is composed of molecules, but neon gas is composed of individual atoms. The molar mass of N2 (g) is greater than that of Ne (g). The N, (g) particles have a greater average kinetic energy than the Ne(g) particles. D. There are more gas particles in tank Y than in tank X