M6L2 Engineering a Better Airbag 2022

when you open a can of soda that has just been shaken, the contents will spray out. This spraying is an illustration of which gas law? 1. Boyles Law 2. Avogards Law 3. Charles Law

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.…

Mg + 02 --> Mgo 13. Balance the following equation: Your answer 14. Using the equation in number 13, when 0.25 moles of Mg reacts with excess oxygen, how many moles of MgO are produced? (Hint: 1 step conversion) * 0.50 moles MgO 0.25 moles Mgo 1.0 moles MgO 0.75 moles Mg0 15. What is the pressure of a 2.0L container that holds 0.78 moles of hydrogen gas at 34 degrees Celsius? (R=0,0821 L atm/K mol),* 9.8 atm 1.09 atm 4.35 atm 39.3 atm

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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Gas Laws A 20.0-L sample of argon gas at 273 K is at atmospheric pressure, 101.3 kPa. The temperature is lowered to 120 K, and the pressure is increased to 145 kPa. a. What is the new volume of the argon sample? b. Find the number of moles of argon atoms in the argon sample. c. Find the mass of the argon sample. The molar mass, M, of argon is 39.9 g/mol.

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?

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

I need hand written solution only

4. Suppose a gas mixture used for anesthesia contains 4.00 mol oxygen (O₂) and 6.00 mol nitrous oxide (N₂O). The total pressure of the mixture is 2.00 atm. a. A mole fraction is defined as the moles of a specific component divided by the total number of moles present. What is the mole fraction of N₂O in this mixture? b. What is the partial pressure in atm of O₂ in this mixture? c. What is the partial pressure in atm of N₂O in this mixture?   5. A gas is formed in the reaction shown below. The gas laws can help determine the volume of gas produced. Zn(s) + 2 HCl(aq) → ZnCl₂ + H₂(g) a. In the last part, you determined that you started with 2.001 moles of Zn. How many moles of H₂ gas will be formed in this reaction? b. At STP, what volume in L of H₂ will be produced? Remember the gas constant, R, is 0.08206 L･atm/mol･K.   6. When the ideas from Boyle’s Law, Charles’ Law and Gay-Lussac’s Law are combined, you get the combined gas law. This law combines the effects of pressure, temperature…

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.

Consider an ideal gas in a closed container of constant volume, which of the following will increase the pressure of the gas?   I. Shaking the container  II. Cooling the system  III. Pumping more gas molecules into the container   Consider an ideal gas in a closed container of constant volume, which of the following will increase the pressure of the gas?   I. Shaking the container  II. Cooling the system  III. Pumping more gas molecules into the container   I and III II only I and II I only

Part B (ii)

Pls help ASAP and pls show all steps. PLS ASAP

I. What is Ideal Gas Law2. Give the different Laws.(6 laws)3. Give practical examples of each law.4.Which one is your favorite type. Why? Original examples if its possible.

CHAPTER 4 GASES Multiple-Choice Questions 1. Determine the density of NO gas at 101 kPa and 35 °C ing dm³. A 0.012 BO.S2 C1 82 D 16 A gas sample contains 42 g nitrogen and 44 g carbon dioxide at a total pressure of 150 kPa. What is the partial pressure of carbon dioxide? A 60 kPa B 76 7 kPa C 90 kPa D 112.5 kPa 2. A sample of gas has a rolume of 430 cm3 at 10 °C and 100 kPa What is the volume of the gas at 30 °C and 110 kPa? A 44 cm³ B 365 cm C 419 cm' D1173 cm Page 1 I 2 Q +

The reaction of 50 mL of N2 gas with 150 mL of H2 gas to form ammonia via the equation:                      N2 (g) + 3H2 (g) → 2NH3 (g) will produce __________ mL of ammonia if pressure and temperature are kept constant.

Which of the following statements about ideal gases is INCORRECT?   a. Ideal gases exist under the assumption of the absence of intermolecular forces. b. Molecules of ideal gases move in constant, random, straight-line motion. c. The ideal gas law describes all the simple gas laws (Boyle's Law, Charles' Law, and Avogadro's Law). d. All gases are ideal at standard temperature and pressure (STP).

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