### Question 7A sealed 99 m³ tank is filled with 6000 moles of ideal oxygen gas (diatomic) at an initial temperature of 270 K. The gas is heated to a final temperature of 320 K. The atomic mass of oxygen is 16.0 g/mol. The mass density of the oxygen gas, in SI units, is closest to:- 3.9- 1.9- 1.5- 2.4- 0.97#### Explanation:To determine the closest mass density of the oxygen gas, you can use the data provided from the problem.For reference: \[\text{Density} (\rho) = \frac{\text{mass}}{\text{volume}}\]Mass can be calculated using the number of moles and the atomic mass:\[\text{Mass} = \text{moles} \times \text{molecular mass}\]Given:- Volume \( V = 99 \, m^3 \)- Moles \( n = 6000 \) moles- Molecular mass of O\(_2\) (since it is diatomic) = \( 2 \times 16 = 32 \, g/mol = 0.032 \, kg/mol \)So, the mass of the gas is:\[\text{Mass} = 6000 \, \text{moles} \times 0.032 \, \text{kg/mol} = 192 \, \text{kg}\]Finally, density is:\[\rho = \frac{192 \, \text{kg}}{99 \, m^3} \approx 1.939 \, kg/m^3\]The closest value to this result is 1.9, so the correct answer is:- 1.9

Answered: Image /qna-images/answer/f4ac4eb1-f486-4cf2-b60f-b5775fb778ec.jpg

A sealed 99 m3 tank is filled with 6000 moles of ideal oxygen gas (diatomic) at an initial temperature of 270 K. The gas is heated to a final temperature of 320 K. The atomic mass of oxygen is 16.0 g/mol. The mass density of the oxygen gas, in Sl units, is closest to:

A sealed 99 m3 tank is filled with 6000 moles of ideal oxygen gas (diatomic) at an initial temperature of 270 K. The gas is heated to a final temperature of 320 K. The atomic mass of oxygen is 16.0 g/mol. The mass density of the oxygen gas, in Sl units, is closest to:

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...

See similar textbooks

Similar questions

The number density in a container of neon gas is 4.80×1025 m^−3. The atoms are moving with an rms speed of 680 m/s . What is the pressure inside the container? p= 2.46×105 Pa What is the temperature inside the container?
The volume of an automobile tire is 2.5 × 10−2m3 . the pressure of the air in the tire is 3 atm and the temperature is 37C ◦ . what is is the mass of air in grams ? The mean molecular mass of air is 29g. 1 atm = 1.01 × 105 Pa ; Calculate to 2 decimals.
The total translational kinetic energy of the molecules of a sample of gas at 415 K is 17500 J. How many moles n does the sample comprise? mol n = Find the average translational kinetic energy Ky of a single molecule. J Kav
Four tanks A, B, C, and D are filled with monatomic ideal gases. For each tank, the mass of an individual atom and the rms speed of the atoms are expressed in terms of m and Vrms respectively (see the table). Suppose that m = 2.68 × 10-26 kg, and Vrms = 1000 m/s. Find the temperature of the gas in each tank. Mass Rms speed A m Urms B m 20rms C 2m Urms D 2m 2Urms
A sample of argon gas is in a container at 35.0° C and 1.22 atm pressure. The radius of an argon atom (assumed spherical) is 0.710 x 10-10 m. calculate the available volume for each atom.
Problem #1: An ideal gas of initial volume V=1m^3, initial temperature T=1000C and initial pressure P=10,000 Pa is heated up to a final temperature T=3000C and allowed to expand into a final volume V=3m^3. What is the final pressure?
Suppose a tank contains 521 m³ of neon (Ne) at an absolute pressure of 1.01×105 Pa. The temperature is changed from 293.2 to 294.4 K. What is the increase in the internal energy of the neon?
Container A contains an ideal gas at a pressure of 5 × 10° Pa and at a temperature of 300 K. It is connected by a thin tube to container B which is four times the volume of A, and contains the same ideal gas at a pressure of 1 x 105 Pa at a temperature of 400 K. The connecting valve is opened, and equilibrium is achieved at a common pressure while the temperature of each container is kept constant at its initial value. What is the final pressure in the system?
Problem 3. The viral coefficients of a gas at 20 °C and 11.5 bar are B = -138 cm³ mol¹ and C=7222 cmº mol². Calculate the V (molar volume) Z (compressibility factor) of the gas. Use the equation below (R = 83.14 cm³ bar mol-¹ K-¹). PV 2 = ² = (1 + = + =) Z RT
0.52 mol of argon gas is admitted to an evacuated 3.00 liter (3.00 × 10-3 m3) container at 20.0°C. The gas then undergoes an isobaric process to a temperature of 260°C. What is the final pressure of the gas, in atm? Your answer needs to have 3 significant figures, including the negative sign in your answer if needed. Do not include the positive sign if the answer is positive. No unit is needed in your answer, it is already given in the question statement.