AOS2 Discussion Activity #1

Time Left:0:55:00 A student completes the experiment The Universal Gas Constant and obtains the following data for one trial. mass of magnesium (g): Initial gas volume (ml): Final Volume (mL): Temperature (°C): Atmospheric pressure (inHg): Ah (cm of water): F3 80 모 Calculate the partial pressure of hydrogen, PH2, for this trial. Give your answer in torr (mmHg). 1 in Hg = 25.4 mmHg 1 cm water = 0.735559 mmHg 1 mol Mg = 24.305 g Mg TABLE D-4 TEMP 1_DEG₁_C_1 1 3 I 1 1 Q F4 0 1 = 2 3 4 5 6 7 8 10 11 12 13 14 0.0 0.1 0.0326 0.00 35.30 21.3 30.21 16 17.13 F5 6.100 | 6.143 1 6.544 1 6.589 0.2 1 VAPOR PRESSURE OF HATER 0-30 DEG. C IN MM HG 1 4.579 4.612 4.646 | 4.924 | 4.959 4.995 15.291 4.660 4.714 5.0315.068 5.329 5.367 5.406 5.445 4.7484.783 4.818 5.104 | 5.141 | 5.178 5.484 5.523 5.563 5.888 5.930 6.230 16.274 6.318 5.363 15.683 15.723 | 5.764 | 5.8051 5.146 6.186 6.636 5.972 1 6.0141 6.057 1 6.407 1 6.453 6.498 1 6.82 | 6.729 6.776 6.823 | 6.871 | 6.919 | 6.967 1 T T 1 I T I 1 17.0167,064…

In an adult human, fully expanded lungs have a total lung capacity (TLC) of about 6 L. Some air remains after complete exhalation, and this volume is the functional residual capacity (FRC). A specific person has a known functional residual lung capacity (FRC) of 2.53 L and a total lung capacity (TLC) of 5.06 L. This person is in a room with an atmospheric pressure of 758.2 mmHg. Their internal temperature is 37.20 °C. How many moles of gas are exhaled with each breath? 1 4 7 0.298 moles 2 5 8 3 6 9 X с

Answer!!!!!

A student completes the experiment The Universal Gas Constant and obtains the following data for one trial. mass of magnesium (g): Initial gas volume (ml): Final gas volume (ml): Temperature (°C): Atmospheric pressure (inHg): 30.39 Calculate the universal gas constant, R, for this trial. Assume that the water levels inside and outside the eudiometer tube are the same; that is, assume Ah = 0.00 cm water. Give your answer to two decimal places in the units of L-torr-mol-1. K-¹. 1 in Hg = 25.4 mmHg 1 cm water = 0.735559 mmHg 1 mol Mg = 24.305 g Mg on i TABLE D-4 TEMP DEGA C T 0 1 2 3 4 amm 14.579 4.612 4.646 | 4.660 4.714 4.924 4.959 4.9955.031 15.068 5.291 5.329 5.367 5.406 15.445 15.683 5.723 | 5.7645.805 5.146 16.100 1 6.143 6.1866.2306-274 1 6.318 10.6 I 0.7 J L 1 LI 1 4.7484.783 4.818 1 4.853 I 4.888 1 5.104 | 5.141 | 5.178 5.216 | 5.253 5.484 5.523 5.563 1 5.60215.647 I 5.888 | 5.930 | 5.972 1 6.014 1.6. 7_1 5.363 | 6.407 6.453 I 6.498 1 6.823 | 6. 871 6.919 1 6.967 1 1 | 6.544 |…

2.) It’s a bad day in the lab!  Two students are doing experiments.  Each is 20 feet away from the professor.  At the same time, each of them lets the same amount of a smelly gas into the room.  One of them releases ammonia, NH3, and the other releases SO2.  NH3 has a pungent odor, and SO2 smells like rotten eggs.  The professor has no idea that this has happened, until she smell the first gas.  Which chemical will the professor smell first?   (NH3 or SO2)                                .  If the professor starts to smell the first gas 42. seconds after the gas is released, how long will it take her to smell the second gas?       sec. * Note: It is unsafe practice to work with these chemicals in an open lab.

Clker-Free-Vector-Images from Pixabay: https://pixabay.com/vectors/balloon-birthday-balloon-25734/ It's 32°F (0°C) outside under normal atmospheric conditions (1 atm) at a stunt performer's birthday party. There is a huge blue balloon filled with flammable hydrogen (H2, molar mass = 2.02 g/mol) gas that she plans to safely ignite, causing a massive explosion. Inside the balloon is 209 g of H2(g). What is the volume of the balloon, in liters? Round to the nearest whole number.

Please send me the question in 20 minutes it's very urgent plz

The global average ozone is approximately 300 DU. At 1atm and 0°C this is equivalent to _ mm thick. Answer:

Its one question with three parts

Please help me on the analysis question. Thank you.

Solid ammonium chloride, NH Cl, is formed by the reaction of gaseous ammonia, NH3, and hydrogen chloride, HCl. NH3(g) + HCl(g) - NH4Cl(s) A 3.87 g sample of NH3 gas and a 3.87 g sample of HCl gas are mixed in a 0.50 L flask at 25 °C. Identify the limiting reagent. HC1 NH3 Q NHẠCH How many grams of NH4Cl will be formed by this reaction? locx mass: 5.9 Incorrect PSY215 Syllabu....docx A Sample Paper_P....pdf ^ MacBook Air 4 Attempt 3 Sample Paper_P....pdf Show All X

Is it possible to get a answer in 20 min?   Explain how you know 3 moles of gas were contained at the maximum volume of 66.2 L. Use the data tables to explain how you knew.    Hint!! the airbag popped above 66.2, the only ones that protected the crash test dummy and didn't pop was 66.2 L.    66.2 is your evidence

Explain the general change in •OH concentration over the course of a day. Why is it greatest at midday and lowest overnight? Please include one or more chemical reactions as part of your answer.

The average molecular speed in a sample of O3 gas at a certain temperature is 362 m/s. The average molecular speed in a sample of O3 gas is ___? m/s at the same temperature. Please don't copy paste  Please write to text formet

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How will the unknown’s reported molar mass be affected in each of the following cases  The atmospheric pressure is recorded too high. A small piece of the foil cap was lost before the final mass was measured.  Condensed water vapor from the bath was trapped underneath the foil cap. The vapor’s volume is assumed to be 125 mL (marked on the side of the flask) instead of the measured volume of the flask. Heating the flask too long resulted in air outside the flask entering and displacing some of the vapor inside the flask. The thermometer is miscalibrated and reads a constant amount too low over its entire temperature range.

Part IV:  Relationships Between Gas Variables   Scientists in the late 1800’s noted relationships between many of the state variables related to gases (pressure, volume, temperature), and the number of gas particles in the sample being studied.  They knew that it was easier to study relationships if they varied only two parameters at a time and “fixed” (held constant) the others.  Use the simulation (PhET) to explore these relationships.   Variables Constant Parameters Relationship Proportionality (see hint below) pressure, volume Pressure- 11.8 atm Particle- 100 Inversely proportional directly proportional or inversely proportional volume, temperature     directly proportional or inversely proportional volume, number of gas particles     directly proportional or inversely proportional   Hint: A pair of variables is directly proportional when they vary in the same way (one increases and the other also increases).  A pair of variables is…

2. What would be the effect on the molar volume if oxygen instead of hydrogen gas (as in equation below) had been collected during this experiment? Explain your answer. MnO2 2H2O2 2H2O O2