5. Does the pressure-volume relationship follow the ideal gas law PV=nRT(is PV constant at constant n and T)Using the room temperature calculate the number of moles in thepressure/volume experiment when the pressure is 1.00atm in 3.1

To calculate the number of moles in the pressure/volume experiment, we can ideal gas law, which is…

Answered: 5. Does the pressure-volume…

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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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…
Starting with Charles's law (stated as an equation), obtain an equation for the final volume of a gas from its initial volume when the temperature is changed at constant pressure. From Charles's law, VT = constant Because this is true for initial conditions as well as for final conditions, we can write V. V; T T; Thus, the equation for the final volume is P.V = P;V; Drag and drop your selection from the following list to complete the answer: P T; V, = V, x Pr PV = constant V = constamt T VT = V;T, V, = V, x T = constant V. P;V; P V, = V, x P, PV = constant T T
A mixture of Oxygen and Chlorine gases contain twice as much Oxygen (by mass - in grams) as Chlorine (2xO2g= Cl2g) If the total pressure of the mixture is 565mmHg, then what is the partial pressure of chlorine ? Using (from Ideal Gas law - Dalton) Partial Pressure Partial Pressure (?) Moles of Chlorine (?) / (divided) by Total Moles O2+Cl2 or written nA / nT (Total Pressure) I've tried to determine what multiple of Oxygen, in grams - by atomic mass, will give me 1/2 the weight of Chlorine - in order to determine Mole (mol) Count for each DIATOMIC. I'm not frustrated, but i'm a little tired of going through this, for 2 hours, I have looked at - similar formula - variations, but this is the challenge. thanks
Sketch three isochores for the same gas at three different volumes V1, V2 and V3 where V1 = V3 and V2<V3. How the temperature scale (K vs oC) will change on your plot?
5. There are 1.07 X 103 moles of gas molecules contained in a CO2 cartridge under 5.0-atm of internal pressure. After several uses, the internal pressure is 3.4-atm. How many moles of gas remain in the cartridge? How much gas will remain in the cartridge when the internal pressure equilibrates to standard pressure? (Assume that the temperature and volume remain constant.)
The ideal gas law is a limiting law, in that it is expected to hold as pressure approaches zero. Suppose the following measured values have been obtained for oxygen gas at 273.15K. Based on the data, calculate R for each pressure value and create a table of pressure and R values (i.e. you are treating R as a variable rather than a constant at this point). Then create a plot R vs p and find the “best value” of R by determining the y-intercept of a straight line fit. (Be sure to label your axes including units).
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.
Determine the mole fraction of toluene if 5.3287 g of toluene, C7H8, was mixed with 6.09 g of cyclopentene, C5H8. MW(C7H8) = 92.141 g/mol; MW(C5H8) = 68.119 g/mol.
CHEM 1 Please solve correctly and give the complete solution.
The average kinetic energy of the molecules in a gas sample depends only on the temperature, T. However, given the same kinetic energies, a lighter molecule will move faster than a heavier molecule, as shown in the equation for rms speed 3 RT rms speed where R = 8.314 J/ (mol·K) and M is molar mass in kilograms per mole. Note that a joule is the same as a kilogram-meter squared per second squared (kg-mIs²). What is the rms speed of O, molecules at 307 K? rms speed: m/s What is the rms speed of He atoms at 307 K? rms speed: m/s
The average kinetic energy of the molecules in a gas sample depends only on the temperature, T. However, given the same kinetic energies, a lighter molecule will move faster than a heavier molecule, as shown in the equation for rms speed 3RT rms speed = where R = 8.314 J/(mol·K) and M is molar mass in kilograms per mole. Note that a joule is the same as a kilogram-meter squared per second squared (kg-m²/s²). What is the rms speed of Cl, molecules at 371 K? rms speed: m/s What is the rms speed of He atoms at 371 K? rms speed: m/s
Using the ideal gas law (PV=nRT), calculate the temperature of a gas in a canister 10.4 L in volume. The pressure is 234,567 Pa and there are 32 moles. (R= 0.0821 L atm/ mol K) (101,325 Pa/1 atm).

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5. Does the pressure-volume relationship follow the ideal gas law PV=nRT (is PV constant at constant n and T) Using the room temperature calculate the number of moles in the pressure/volume experiment when the pressure is 1.00atm in 3.1