QUESTION 2Once you have completed the first measurement, increase the temperature till it has doubled. Use the bucket below to create fire.Your answer will be values for all four gas properties, separated by a comma. Provide the values for the first three properties you set by adjusting the simulation: P, V and T. SeeInstructions on how to find the values. For the fourth value, n (moles), calculate using the moles using the Ideal Gas Law formula in the directions. Answer will have the format,Pressure (atm), Volume (L), Temperature (K), Moles.For example, one possible answer is,33.9 atm, 100.0 L, 501 K, 83 molesTTTT ParagraphArlalv (12pt)v = - E - T p-QTao0 田HTML CSSJ.O MashupsWords:0Path: p Description You will use an online simulation to manipulate and calculate the four properties of gases: Pressure, Volume, Quantity, and Temperature. You will also apply your knowledge to several scenarios.To begin, open the simulation, Gases Intro, from https://phet.colorado.edu/sims/html/gases-intro/latest/gases-intro en.html. This will open it in another window. Select the simulation box Intro at the bottom. Whenit opens, check Width to show the width of the box. You should leave the rest unchecked. We will only use Heavy Particles. Play around with the simulation to see how to adjust the volume/width (handle on left ofbox), temperature (bucket below with either ice or fire), and quantity (using the pump handle to right of the box). Keep the box sealed by keeping top door closed. When you are ready to do the experiments,reset the simulation by pressing the white eraser button on bottom right, make sure width is 10.0 nm, and set to heavy particles (purple gas molecules).Instructions To do first experiment, pump the gas pump to put gas into the chamber. Only use between 3 and 7 pumps. Increase the temperature to a number you like between 100 K and 500 K, using the fire/ice bucket onbottom. Do not change the chamber width for now, keep it at 10.0 nm (handle on left of chamber). Do not open the chamber to let gas molecules out (handle on top of chamber).Calculating moles using the Ideal Gas Law: PV nRT, where R = 0.0821Once you have everything how you like it, you will calculate how many moles of gas are in the chamber, by using the Ideal Gas Law. Recall the Ideal Gas Law requires specific units: atm, L, moles, and Kelvin.PressureIs indicated by the circular instrument on the top right of the chamber. It is conveniently already in atmospheres.Volume - Determine the volume in nm^3 by multiplying the width, height, and depth of the chamber. Depth is always 1.00 nm and height is always 10.0 nm. Width is adjusted by you to 10.0 nm or 15.0 nm,depending on the experiment. Volume then is: width you adjust X 10.0 nm X 1.00 nm. Simplifying, it is the width you select X 10.0, with units of nm^3. To simplify calculations assume your volume answer in nm^3 areactually Liters (L), when calculating the Ideal Gas Law.Temperature- This is indicated by the thermometer, conveniently already in units Kelvin.Quantity-for these experiments you will be calculating the quantity, or moles, of gas under each scenario. What is the solution when you solve the Ideal Gas Law, PV=nRT, for n, moles? R = 0.0821.

The main aim of this question explain the relationship between pressure, volume, temperature and…

QUESTION 2 Once you have completed the first measurement, increase the temperature till it has doubled. Use the bucket below to create fire. Your answer will be values for all four gas properties, separated by a comma. Provide the values for the first three properties you set by adjusting the simulation: P, V and T. See Instructions on how to find the values. For the fourth value, n (moles), calculate using the moles using the Ideal Gas Law formula in the directions. Answer will have the format, Pressure (atm), Volume (L), Temperature (K), Moles. For example, one possible answer is, 33.9 atm, 100.0 L, 501 K, 83 moles

QUESTION 2 Once you have completed the first measurement, increase the temperature till it has doubled. Use the bucket below to create fire. Your answer will be values for all four gas properties, separated by a comma. Provide the values for the first three properties you set by adjusting the simulation: P, V and T. See Instructions on how to find the values. For the fourth value, n (moles), calculate using the moles using the Ideal Gas Law formula in the directions. Answer will have the format, Pressure (atm), Volume (L), Temperature (K), Moles. For example, one possible answer is, 33.9 atm, 100.0 L, 501 K, 83 moles

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

Chapter5: Gases

Section: Chapter Questions

Problem 130E

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Analyze When nitroglycerin (C3H5N3O9) explodes, itdecomposes into the following gases: CO2 , N2 , NO, and H2O . If 239 g of nitroglycerin explodes, what volumewill the mixture of gaseous products occupy at 1.00 atmpressure and 2678°C?
Please help me on the analysis question. Thank you.
(References] Use the References to access important values if needed for this question. A sample of xenon gas at a pressure of 0.949 atm and a temperature of 26.9 °C, occupies a volume of 11.0 liters. If the gas is compressed at constant temperature to a volume of 3.30 liters, the pressure of the gas sample will be Submit Answer Try Another Version 3 item attempts remaining Previous Next Email Inst Cengage Learning | Cengage Technical Support AP DELL
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Use the theoretical number of moles of H2 from #1, the partial pressure of H2 from #2, the volume of H2 gas collected (in L), and the temperature (in K) to find the experimental value of the universal gas constant (R):
naining Time: 43 minutes, 12 seconds. estion Completion Status: QUESTION 20 In the experiment "Molar mass of volatile liquid", the pressure of the gas inside a flask was the same as atmosphere, and the temperature was identical to the boiling water temperature of water bath. How did you measure the volume of the gas inside the flask? - O Read the volume written on the flask. Fill the flask up to the brim with water and then transfer the water to a graduated cylinder. Measure the volume of the liquid added to the flask before heating the sample. Measure the volume of the liquid that condenses in the flask after cooling the sample. QUESTION 21 Name the laboratory equipment. Save All Click Save and Submit to.save and submit. Click Save All Answrers to save all anstcers
Since volume and pressure are inversely related, we can make some assumptions about initial and final states using the data provided. We can also identify initial and final states by finding trigger words in the language of the problem. Look for words like “first,” “initially,” or “originally” to describe initial states and “result” or “after” for final states. What volume would a sample of helium occupy at 6.0 atm if the helium was initially compressed in a 1.0 L tank at 20. atm at constant temperature? Organize your data into the table to help analyze the problem. Leave blank any boxes for which you do not have information. Drag the appropriate labels to their respective targets.
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