Gases Workshop Activity - Oct 3rd_4th (Workshop 6)

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10/4/22, 12:46 PM Gases Workshop Activity - Oct 3rd/4th (Workshop 6) https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=11224673 1/25 Gases Workshop Activity - Oct 3rd/4th (Workshop 6) Due: 12:00am on Monday, December 12, 2022 You will receive no credit for items you complete after the assignment is due. Grading Policy Exercise 6.26 - Enhanced - with Feedback MISSED THIS? Read Section 6.2 (Page) . The pressure on top of Mount Everest (29,029 ) averages about 235 . Part A Convert this pressure to . ANSWER: Correct The units of and are equivalent. This means that 235 is equal to 235 . Part B Convert this pressure to . ANSWER: Correct Converting from to requires two steps. The first is to convert to , and the second is to convert to . Part C Convert this pressure to . ANSWER: Correct The pressure in is converted to the pressure in by dividing by 760. The pressure in is then determined by multiplying by 29.92. Part D Convert this pressure to . ANSWER: Correct Converting to is a one-step conversion that involves dividing by 760. Exercise 6.33 - Enhanced - with Feedback and Hints = 235 = 4.55 = 9.25 = 0.309
10/4/22, 12:46 PM Gases Workshop Activity - Oct 3rd/4th (Workshop 6) https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=11224673 2/25 MISSED THIS? Read Section 6.3 (Page) ; Watch KCV 6.3 . A 48.5 sample of gas in a cylinder is warmed from 20 to 84 . Part A What is its volume at the final temperature? (Assume constant pressure.) Express your answer in millililters to three significant figures. Hint 1. Convert between degrees Celsius and kelvins The temperature values used in the simple gas laws are in kelvins. Convert the initial and final temperatures of the sample to kelvins. Express your answers in kelvins to three significant figures separated by a comma. ANSWER: ANSWER: Correct Charles's law is where and are the initial volume and temperature of the gas and and are the final volume and temperature. Solving this equation for gives Before substituting the numerical values to calculate , convert the initial and the final temperatures to kelvins . Substitute , , and to calculate : Exercise 6.32 - Enhanced - with Feedback MISSED THIS? Read Section 6.3 (Page) ; Watch KCV 6.3 . A sample of gas has an initial volume of 14.3 at a pressure of 1.20 . Part A If the sample is compressed to a volume of 10.5 , what is its pressure? Express the pressure in atmospheres to three significant figures. ANSWER: , = 293,357 = 59.1 = 1.63
10/4/22, 12:46 PM Gases Workshop Activity - Oct 3rd/4th (Workshop 6) https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=11224673 3/25 Correct Boyle’s law ( ) relates the initial and final pressures and volumes of a gas when the number of moles and temperature remain constant during compression (or expansion). The calculation of the final pressure is summarized as follows: Exercise 6.35 - Enhanced - with Feedback and Hints MISSED THIS? Read Section 6.3 (Page) ; Watch KCV 6.3 . A balloon contains 0.110 of gas and has a volume of 2.90 . Part A If an additional 0.118 of gas is added to the balloon (at the same temperature and pressure), what will its final volume be? Express your answer in liters to three significant figures. Hint 1. Calculate the total moles of gas 0.118 of gas is added to the balloon containing 0.110 of gas (at the same temperature and pressure). Calculate the final number of moles of gas. Express your answer in moles to three significant figures. ANSWER: ANSWER: Correct If the number of moles of gas in a balloon increase at a constant temperature and pressure, its volume increases in direct proportion, as the greater number of gas particles fill more space. This statement can be mathematically described by Avogadro's law: Solve this equation for the final volume from the initial volume ( ), initial number of moles ( ) and final number of moles ( ): The total number of moles of gas particles isS Substituting and the given quantities to calculate gives Exercise 6.37 - Enhanced - with Feedback and Hints = 0.228 = 6.01
10/4/22, 12:46 PM Gases Workshop Activity - Oct 3rd/4th (Workshop 6) https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=11224673 4/25 MISSED THIS? Read Section 6.4 (Page) ; Watch KCV 6.3 , IWE 6.5 . Part A What volume is occupied by 0.103 of helium gas at a pressure of 0.94 and a temperature of 302 ? Express your answer using two significant figures. Hint 1. Rearrange the ideal gas law to solve for volume You are given a temperature ( ), pressure ( ), and the number of moles ( ) of helium and asked to solve for the unknown volume ( ). The ideal gas law relates all the given conditions. Rearrange the ideal gas law to solve for . Express your answer in terms of , , , and . ANSWER: ANSWER: Correct Rearrange the ideal gas law to solve for the unknown volume ( ). The temperature ( ) and pressure ( ) are given in the correct units of kelvin ( ) and atmospheres ( ). The moles ( ) of helium gas are given. Use the gas constant so that the units of atmospheres, kelvins, and moles cancel, leaving only the desired units of liters ( ). Substitute the given values into the ideal gas law and solve for volume. Part B Would the volume be different if the gas was argon (under the same conditions)? Match the words in the left column to the appropriate blanks in the sentences on the right. ANSWER: = = 2.7 Reset Help different The volume would be the same if the gas was argon because the ideal gas law is dependent on the number of moles of the gas and not the mass .
10/4/22, 12:46 PM Gases Workshop Activity - Oct 3rd/4th (Workshop 6) https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=11224673 5/25 Correct The ideal gas law given below is used to calculate the volume of a gas. The terms , , , and represent the pressure, volume, number of moles, and temperature, respectively. The terms represents the gas constant. Notice that the moles of a gas are what is used in the calculation for volume, not the mass of the gas. Therefore, as long as the number of moles of gas remains constant, along with the other given conditions, the volume also remains the same. Thus, the gas law is dependent on the number of moles of gas not the mass of a gas. Exercise 6.44 - Enhanced - with Feedback MISSED THIS? Read Section 6.4 (Page) ; Watch KCV 6.3 , IWE 6.5 . Part A A weather balloon is inflated to a volume of 29.7 at a pressure of 733 and a temperature of 26.3 . The balloon rises in the atmosphere to an altitude where the pressure is 385 and the temperature is -15.7 . Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude. ANSWER: Correct The number of moles in the weather balloon will remain constant. According to the ideal gas law, the changes in pressure and temperature will cause a change in volume. Volume and pressure are inversely related, while volume and temperature are directly related. Exercise 6.40 - Enhanced - with Feedback MISSED THIS? Read Section 6.4 (Page) ; Watch KCV 6.3 , IWE 6.5 . Part A What is the pressure in a 23.0- cylinder filled with 49.9 of oxygen gas at a temperature of 331 ? Express your answer to three significant figures with the appropriate units. ANSWER: Correct The pressure can be solved for using the ideal gas equation ( ). The moles of oxygen must be determined using the molar mass of molecular oxygen, ( ). Exercise 6.54 - Enhanced - with Feedback MISSED THIS? Read Section 6.5 (Page) . Part A = 48.6 = 1.84
10/4/22, 12:46 PM Gases Workshop Activity - Oct 3rd/4th (Workshop 6) https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=11224673 6/25 Use the molar volume of a gas at STP to calculate the density (in ) of oxygen gas at STP. Express the density in grams per liter to three significant figures. ANSWER: Correct The standard molar volume of a gas is 22.414 , and the molar mass of is 32.00 . The density is found by dividing the mass of a gas by its volume: . Therefore, you can divide the molar mass of a gas (in grams per mole) by its molar volume (in liters per mole) to determine its density (in grams per liter). Exercise 6.55 - Enhanced - with Feedback and Hints MISSED THIS? Read Section 6.5 (Page) ; Watch IWE 6.7 . Part A What is the density (in ) of hydrogen gas at 24 and a pressure of 1645 ? Express your answer in grams per liter to three significant figures. Hint 1. Derive the equation for density from the ideal gas law Because density is a mass per unit volume, and because molar mass is the mass per mole, the density of a gas is its molar mass ( ) divided by its molar volume (moles ( ) per volume ( )): By substituting these into the ideal gas law where is pressure, is the ideal gas constant, and is temperature, derive the general equation for the density of a gas ( ) that can be used to calculate the density under any conditions. Express your answer in terms of , , , and . ANSWER: ANSWER: = 1.43 = = 9.25
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