M6L2 Engineering a Better Airbag 2022

69 * 00 < CO T R #3 Your answers are saved automatically. Remaining Time: 13 minutes, 21 seconds. * Question Completion Status: 2 1. 3. QUESTION 1 A mixture of three gases, Ron, Harry and Hermione is stored in a constant volume container at constant temperature. The mixture contains the amount of moles of each of these gases listed below. The total pressure of the mixture is 3.95 atm. What is the partial pressure (atm) of Gas Ron in the mixture? Report your answer to the thousandths place and do not include units. Ron Harry He mione 0.696 mol 0.724 mol 0.338 mol QUESTION 2 The heat of combustion for C3H8 (44.1 g/mol) is -2220.0 kJ/mol. Calculate the heat of reaction (in kJ) when 14.88 g C3H8 is combusted. Be sure to include the correct sign in your answer (+ or -) and do not put a space between the sign and the number. Do not include units in your answer. Report your answer to the hundredths place. Click Save and Submit to save and submit. Click Save All Answers to save all answers.…

Kiki, Karl’s twin sister, did a lab just like our butane lab. But she did not have butane  as her gas. Use the Ideal Gas law to help Kiki determine the molecular mass of the  gas from the following data. A sample of a gas is collected by water displacement.  ➢ The mass of the gas cylinder before releasing the gas is 25.00g. ➢ The mass of the gas cylinder after releasing the gas is 21.08g.  ➢ The volume of the gas is 3.35 L.  ➢ The barometric pressure is 740.2mmHg.  ➢ The room temperature is 28.0ºC and

Part 1: Gas Laws The physical properties of gases can be explained using four variables; volume (V), pressure (P), temperature (T), and amount in number of moles (n). Four simple laws are used to explain the behavior of gaseous species. Complete the table below to summarize the four gas laws. Name of the gas Properties that Properties that Gas law equation Gas law explanation law stay constant are changing n and T P:V1 = P:V2 Charles's law T and V are directly proportional. (as T increases V also increases) Pand T P1 P2 T1 T2 Avogadro's law V and n

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1. Indicate which conditions would keep the soda fizzy (more H2CO3) by selecting the correct change in the stressor from the drop down menu. Pressure  increases or decreases? Volume    increases or decreases? Amount of CO2    increases or decreases? Temperature    increase or decreases?

Question 4 of 20 The change in distribution of six gaseous particles between three interconnected containers is shown in the images. Determine which of the changes have a positive AS. a Chapter 34-Part 1.pptx a Chapter 34-Part 2.pptx a Chapter 34-Part 2.pptx A The Social Dilem..docx O The Social Dilem.docx

Avogadro's Law This law explains why bread and other baked goods rise. Yeast or other leavening agents cause the production of carbon dioxide gas and ethanol. The carbon dioxide forms bubbles which appear as holes in the dough. As the yeast continues the leavening process, the number of particles of carbon dioxide increases, hence causing an increase in the number, or volume, of bubbles and in the size of the dough. How about inflating a basketball?

Look at the diagram below. What will happen in the piston chamber if more pressure is applied to the piston? T'

Consider the following gas samples:   Sample A Sample B   S2(g) O2(g)     n = 1 mol n = 2 mol     T = 800 K T = 400 K     P = 0.20 atm P = 0.40 atm     Select one: a. The volume of sample A is twice the volume of sample B. b. The average kinetic energy of the molecules in sample A is twice the average kinetic energy of the molecules in sample B. c. The fraction of molecules in sample A having a kinetic energy greater than some high fixed value is larger than the fraction of molecules in sample B having kinetic energies greater than that same high fixed value. d. The mean square velocity of molecules in sample A is twice as large as the mean square velocity of molecules in sample B. e. Assuming identical intermolecular forces in the two samples, sample A should be more nearly ideal than sample B.

Pls help ASAP and pls show all steps. PLS ASAP

Determine the mass of NaClO4 needed to produce 20.0 L of 02 at STP according to the (unbalanced) equation below: NaClO4(s) NaCl(s) + O2(g) (The molar mass for NaClO4 is 122.44 g/mol.) OA.0.45 g O B. 68.6 g OC. 109.3 g O D.0.89 g O E. 54.7 g

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When you allow neon to leak out of a container, the 150ml container empties in 18.6 seconds. When you fill the same container (at the same temp and pressure) with an unknown, it empties in 40.6 seconds. What is the identity of the unknown? a.C2H3Cl b.CH2Cl2 c.C2H2Cl2 d.CHCl3 e.CCl4

. If pressure and temperature are kept constant, the reaction of 18 mL of N2 gas with 54 mL of H2 gas will form ________ mL of ammonia.Given: N2 + 3 H2 → 2 NH3

Fill in the blank   The partial pressure on the surface of Mars is 0.0070 atmospheres. The mole fractions of the top three components in the Martian atmosphere are 0.953 for CO2, 0.026 for N2, and 0.019 for Ar. In terms of torr (1 atm = 760 torr) the partial pressure of CO2 on Mars is ____________ torr, the partial pressure of N2 is  ______________ torr, and the partial pressure of Ar is _______________ torr.

1. In the ideal gas law, R depends on the pressure and temperature of the gas. True or false? 2. When the leveling bulb is higher than the water level, the pressure in the system is greater than atmospheric pressure. T or F? When the leveling bulb is lower than the water level, the pressure in the system is greater than atmospheric pressure. T or F?

Answer part A, B, and C

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1. What mass of helium gas exerts a pressure of 1.20 atm in a volume of 5.40 L at a temperature of 27°C? PV (Hint --- n = Find n, then convert to grams using the molar mass.) RT 2. A 2.50 g sample of neon gas is added to a 5.00 g sample of argon gas in a 10.0-L container at 23°C. Calculate the partial pressure of each gas and the total pressure of the mixture. (Hint--- Convert mass to moles, then use P nRT to find the pressure of both gases. Then add the pressures to find the total pressure.)

1.  Where did the R constant in PV=nRT come from, and why must we convert everything to the units of the R constant? 2.  Why does the density of water change with its temperature? 3.  If all of the gas was not vaporized before taking the mass (some stayed in liquid form), how would that affect the final molar mass calculation? 4. If a sample of ethanol (C2H6O) was determined to have a pressure of 2 atm at a temperature of 25°C, what is its density (in g/L)?

The stopcock connecting a 4.82 L bulb containing oxygen gas at a pressure of 7.91 atm, and a 3.57 L bulb containing neon gas at a pressure of 2.92 atm, is opened and the gases are allowed to mix. Assuming that the temperature remains constant, the final pressure in the system is _______atm.