A technician measures the pressure at 4 locations along a natural gas pipeline, but the gauges at each site use different units. Compare the reported values to determine whether all the pressures are equivalent or whether one site has a pressure different to the others. (Note the choices below may be given in 'exponential' format, e.g. 1200000 = 1.2x106 would be displayed as 1.2e6) - Pressure conversion factors are given in the Module 3 Useful Data page. O 6.18 bar at site B is different O 6.10 atm at site A is different O 618 kPa at site K is different O All pressures are equivalent O 6.18e4 Pa at site P is different

A technician measures the pressure at 4 locations along a natural gas pipeline, but the gauges at each site use different units. Compare the reported values to determine whether all the pressures are equivalent or whether one site has a pressure different to the others. (Note the choices below may be given in 'exponential' format, e.g. 1200000 = 1.2x106 would be displayed as 1.2e6) - Pressure conversion factors are given in the Module 3 Useful Data page. O 6.18 bar at site B is different O 6.10 atm at site A is different O 618 kPa at site K is different O All pressures are equivalent O 6.18e4 Pa at site P is different

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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1. A student following the procedure described in this module collected the following data: mass Mg, g 0.0243 initial syringe volume, mL 1.0 final syringe volume, mL 26.5 barometric pressure, torr 754 temperature, K 298 Determination#1 The value of the gas law constant (R) is 0.0822 L.atm/mol.K Determination #2 he volume of hydrogen gas produced by the reaction of 0.243 g of magnesium metal and collected at 750 torr and 298 K = 248 mL The results of this experiment are greatly affected by the care with which each of the steps is completed (a) Describe the error that would occur if the magnesium were to slide into the HCl in the test tub before the system is sealed off (b) What would be the effect on the results of a rise in the room temperature from 22.0 celcius, when determination #1 was done, to 25.3 celcius, when determination #2 was made? (c) Why must the surface coating of MgO be removed prior to determining the mass of magnesium used in the experiment? (d) What would be the…
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The ideal gas law describes the relationship among the volume of an ideal gas (V), its pressure (P), its absolute temperature (T), and number of moles ( n): PV = nRT Under standard conditions, the ideal gas law does a good job of approximating these properties for any gas. However, the ideal gas law does not account for all the properties of real gases such as intermolecular attraction and molecular volume, which become more pronounced at low temperatures and high pressures. The van der Waals equation corrects for these factors with the constants a and b, which are unique to each substance: (P+ ²) (V-nb) = nRT an² The gas constant R is equal to 0.08206 L.atm/(K-mol). Part A A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 16.0 °C is 2.45 atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask? Express your answer to three significant figures and include the appropriate units. View Available Hint(s) mass of NH3 = Submit ▾ Part B HÅ…
A certain gas mixture is at a pressure of 3500 kPa and is composed of 18.0 g of O2 and 28.0 g of CO2. Determine the partial pressure of O2 gas in the mixture.
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Gases are different from solids and liquids. In a sample of gas, the molecules are far apart. The gas molecules also move around and collide with each other as well as with the walls of the container. These collisions generate pressure. The pressure of a gas can be measured in different units. One convenient unit of measure is called the atmosphere (atm) because it is based on atmospheric pressure. At sea level, the average pressure is 1 atm. As you get higher in altitude, the pressure steadily drops until you leave the atmosphere, where the pressure is very close to 0 atm. The table below shows the different commonly used units of measuring gas pressure. Use this table in the pressure unit conversions. Unit Abbreviation 1 atm equivalent FT atmosphere atm 1.00 atm (exact) millimeters of mercury mmHg 760 mmHg torr 760 torr inches of mercury in. Hg 29.9 in. Hg pounds per square lb/in.² 14.7 lb/in.² inch (psi) pascal torr Pa 101,325 Pa Part A Convert 1.20 atm of pressure to its equivalent…
A sample of oxygen gas was found to have a pressure of 94kPa when the temperature was 19°C. What can its pressure be, in kPa , expected to be if the temperature is 12.5°C? Round off your answer to 2 decimal values
A 10.00 L tank at 5.3 °C is filled with 5.84 g of carbon dioxide gas and 4.39 g of chlorine pentafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Be sure each of your answer entries has the correct number of significant digits. gas carbon dioxide chlorine pentafluoride mole fraction 00 X
In dry atmospheric air, the four most abundant components are N₂, X = 0.808; O₂, X = 0.1915; Ar, X = 9.34x10-5; and CO₂, X = 4.066x104. Calculate the partial pressure of CO₂, in torr, under standard atmospheric conditions. Submit Answer Tries 0/99 This discussion is closed. M CAL 8:00- 10:50- CI 12:00 Q ! 2 @ W OCT 21 F2 # 3 E 80 F3 $ 4 R 10 Q F4 % 5 T F5 A 6 Y F6 tv A S MacBook Air & 7 8 F7 8 DII FB ( 9 F9 O ) 0 J F10 F11 + F12 Send Feedback
The ideal gas law describes the relationship among the pressure P, volume V, number of moles n, and absolute temperature T of an ideal gas. Here is the relationship expressed mathematically: PV = nRT where R is a proportionality constant. The units of R are determined by the units of pressure and volume used in the equation. When bar used for pressure and L for volume, the appropriate R value is 0.08314 L bar mol-¹ K-¹. Part A How many air molecules are in a 4.05 x 3.66 x 3.05 m³ room? Assume atmospheric pressure of 1.00 bar, a room temperature of 20.0 °C, and ideal behavior. Express your answer using three significant figures. ► View Available Hint(s) VE ΑΣΦ + Review | Constants | molecules
1. The compressibility factor Z = PV/nRT for O2 at -27.1°C and 537.1 atm is 1.50; at 147.4°C and 95.5 atm, it is 1.02. A certain mass of oxygen occupied a volume of 3.28 L at 147.4°C and 95.5 atm. Calculate the volume occupied by the same quantity of oxygen at -27.1°C and 537.1 atm. 2. The composition of a mixture of gases in percentage by volume is 20.5% nitrogen, 15.7% carbon monoxide, 37.8% water, and the rest sulfur dioxide. Calculate the density of the gaseous mixture at 39.8°C and 1.46 atm in grams/liter. Report your answer to the hundredths position.
Use the combined gas law by plugging in the numbers into it and solve the missing part