**Problem 8:**A rigid tank contains 73.5 g of chlorine gas (Cl₂) at a temperature of 74 °C and an absolute pressure of 5.30 × 10⁵ Pa.The mass per mole of Cl₂ is 70.9 g/mol. Determine the volume of the tank.[Answer box: _____ liters]**Explanation:**This problem requires determining the volume of the tank by applying the ideal gas law:\[ PV = nRT \]Where:- \( P \) is the pressure (5.30 × 10⁵ Pa)- \( V \) is the volume to be determined- \( n \) is the number of moles of Cl₂- \( R \) is the ideal gas constant (8.314 J/(mol·K))- \( T \) is the temperature in Kelvin (74 °C = 347 K)Calculate the number of moles (\( n \)) using the mass and molar mass of chlorine gas. Substitute the values into the ideal gas law equation to solve for the volume.

Answered: Image /qna-images/answer/4692a460-78b0-4a62-8d97-183ad218ad71.jpg

8. A rigid tank contains 73.5 g of chlorine gas (Cl2) at a temperature of 74 °C and an absolute pressure of 5.30 × 10° The mass per mole of Cl2 is 70.9 g/mol. Determine the volume of the tank. liters 60 ss Pa. 60 ssf60 sf60 ss

8. A rigid tank contains 73.5 g of chlorine gas (Cl2) at a temperature of 74 °C and an absolute pressure of 5.30 × 10° The mass per mole of Cl2 is 70.9 g/mol. Determine the volume of the tank. liters 60 ss Pa. 60 ssf60 sf60 ss

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

Related questions

Q: Nitrogen gas is trapped inside a 4.8L cylinder with a moveable piston at a pressure of 1.0atm. If…

Q: 1. An ideal gas at 20.00C and pressure 1.50x105 Pa is in a container having a volume of 1 litter. a)…

A: Solution:-Given thatInitial temperature (T1)=20°C=20+273=293 KInitial pressure (P1)=1.5×105…

Q: An ideal gas is confined to a container with adjustable volume. The pressure and mole number are…

A: An ideal gas law is confined to a container with adjustable volume.The pressure and mole number are…

Q: an initial volume of an ideal gas is compressed to one-half its original volume, and to twice its…

A: According to question we need to find--- what happens to the pressure after change ?

Q: What is the density of diatomic nitrogen gas (N2) at a temperature of 20.00 C under a pressure of…

A: Given data- For Diatomic nitrogen gas (N2) temperature T= 20.0°C and pressure P=100 kPa The atomic…

Q: PCMRG 273 cm³ of an ideal gas has an initial temperature of 0°C. The gas is heated at a constant…

A: Hi. as you have posted multiple questions and have not specified which question needs to be solved,…

Q: Pure helium gas is contained in a leak-proof cylinder containing a movable piston. The initial…

A: Given: Initial volume V0=15 L, Initial pressure P0=2 atm, Initial temperature T0=310 K, Final volume…

Q: What would be the volume of 3.90 moles of an ideal gas, at STP? What is the pressure of this gas, if…

Q: QUES What is the density in kg/mo of diatomic oxygen gas, 02, that is under a pressure of 100 kPa at…

Q: During inhalation, a person's diaphragm and intercostal muscles contract, expanding the chest cavity…

Q: Question 2 A sample of a gas is in a container. The temperature of the gas is decreased. Based on…

A: Given, The temperature of the gas is decreased. Volume of a container is fixed.

Q: A high-pressure gas cylinder contains 50.0 L of toxic gas at a pressure of 1.25 × 107 Pa and a…

Q: A high pressure gas cylinder contains 45.5 L of toxic gas at a pressure of 1.2X10^7 N/m^2 and a…

A: Since you have uploaded a question with multiple sub-parts, we will solve the first three sub-parts…

Q: 3. The pressure, temperature and volume of an ideal gas are given by the ideal gas law pV = nRT…

Q: 10 moles of an ideal gas are confined to a volume of 2 m^3. What is the temperature of the gas if…

Q: An ideal gas in a sealed container has its volume doubled and its temperature tripled. By what…

Q: 37. (a) What is the gauge pressure in a 25.0°C car tire containing 3.60 mol of gas in a 30.0 L…

A: Given, T0=25.00 Cn=3.60 molV0=60.0 L

Q: Problem 6: Suppose a 26.5°C car tire contains 3.5 mol of gas in a 32.5 L volume. Part (a) What is…

Q: 0.10 mol of Argon gas is admitted to an evacuated 50cc container at 20°C. The gas is then heated at…

A: Given data The initial volume is V1=50 cm3 The initial temperature is T1=20oC The final temperature…

Q: 4. Large helium-filled balloons are used to lift scientific equipment to high altitude. What is the…

A: Helium is an ideal gas. The ideal gas equation is given as,

Q: 18.6 A 0.5 m³ container holds 50 mol of an unknown gas at a temperature of 25 °C. a. At what…

A: Volume of container (V) = 0.5 m3Number of moles (n) = 50 moles Temprature of gas (T) = 25oC = 298…

Q: Gas is confined in a tank at a pressure of 9.2 atm and a temperature of 27.0°C. If two-thirds of the…

A: Initial pressure (Pi) = 9.2 atm Initial temperature (Ti) = 27°C = 300 K Final temperature (Tf) =…

Q: Suppose a 22.5°C car tire contains 3.85 mol of gas in a 32.5 L volume. What is the gauge pressure,…

A: Given, The temperature of the car tire T=22.50C =22.5+273 =295.5 K No; of moles of gas (n) = 3.85…

Q: of an average molecular mass of 29 u. What is the mass of the air in the room at a pressure of 1.0…

A: To calculate the mass of air in the room, we can use the ideal gas law equation:PV = nRTwhere: P =…

Q: 6. A Goodyear blimp typically contains 4900 m² of helium (He) at an absolute pressure of 1.00 x 10°…

A: Using ideal gas law PV=nRTn=PVRT

Q: 3.93 m3 of a gas initially at STP is placed under a pressure of 3.69 atm , the temperature of the…

A: (P1)(V1)/(T1) = (P2)(V2)/(T2) ..............by gas law V2 = (P1)(V1)(T2) / (P2)(T1) where P1 = 1 atm…

Q: A sealed box with volume 2 m^3 contains an ideal gas with 2.0*10^26 particles at a temperature of…

A: Since you are posted more than one question, we will answer the first question. If any specific…

Q: 0.52 mol of argon gas is admitted to an evacuated 3.00 liter (3.00 × 10-3 m3) container at 20.0°C.…

A: Page 1

Q: If 86.5 moles of an ideal gas occupies 0.0275 cubic meters at 39.5 °C, what is the pressure of the…

Concept explainers

Ideal Gas Law

Ideal gas law states that the product of pressure and volume of a gas directly varies with the product of the number of moles, the universal gas constant, and the temperature of the gas.

Question

**Problem 8:**

A rigid tank contains 73.5 g of chlorine gas (Cl₂) at a temperature of 74 °C and an absolute pressure of 5.30 × 10⁵ Pa.

The mass per mole of Cl₂ is 70.9 g/mol. Determine the volume of the tank.

[Answer box: _____ liters]

**Explanation:**

This problem requires determining the volume of the tank by applying the ideal gas law:

\[ PV = nRT \]

Where:
- \( P \) is the pressure (5.30 × 10⁵ Pa)
- \( V \) is the volume to be determined
- \( n \) is the number of moles of Cl₂
- \( R \) is the ideal gas constant (8.314 J/(mol·K))
- \( T \) is the temperature in Kelvin (74 °C = 347 K)

Calculate the number of moles (\( n \)) using the mass and molar mass of chlorine gas. Substitute the values into the ideal gas law equation to solve for the volume.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, physics and related others by exploring similar questions and additional content below.

Similar questions

7) A gas has a volume of 5 cubic feet and a gauge pressure of 3 atm at a temperature 40 degrees Fahrenheit.The volume is decrease to 2 cubic feet and the temperature is raised to 140 degrees Fahrenheit.What is the new gauge pressure in atm’s?
A3] a) Find the temperature of 1 mole of oxygen molecules if they occupy a volume of 4 L and have a pressure of 6 x 10° Pa. You should treat the oxygen as an ideal gas and take the value of the universal gas constant to be R = 8.31J mol1 K-. b) What is the density of the oxygen? You may assume that the mass of I mole of oxygen molecules is 32 g. c) What is the mean square velocity of the oxygen molecules? d) State two assumptions of the kinetic theory of ideal gases that the van der Waals model does not require to be true.
Pr4. The pressure of an ideal gas in a closed rigid container is 0.6 atm at 35 degrees C. The number of molecules is 5×1022 (one mole of gas contains 6 x 1023 molecules and 1 atm = 1.01 × 105 Pa) a) What is the pressure in Pa and temperature in K of the gas? b) How many moles of gas is in the container? c) What is the volume of the container? d) If the container is heated to 120 degrees C, and volume remains the same what is the pressure of the gas in atm?
Gas is confined in a tank at a pressure of 9.2 atm and a temperature of 21.5°C. If two-thirds of the gas is withdrawn and the temperature is raised to 85.0°C, what is the pressure of the gas remaining in the tank? ?atm
63.0 L of oxygen at 21.0°C and an absolute pressure of 2.55atm are compressed to 38.3L and at the same time, the temperature is raised to 53.0°C. What will the new pressure be? P= atm
4. An ideal gas is contained in a vessel of volume 12 L (12 liters) at a temperature of 20 °C and a pressure of 9 atm. a) How many moles of gas are in the vessel? b) How many molecules of gas are in the vessel?
A gas condensed in a cylinder with a nozzle is initially at p_1=2000 Pa, V_1= 2.0 l, and t_1=300 K. a) If the volume decreases to 0.50 L while the temperature remains low, what is the new pressure?b) If in a) the temperature increases to 400 K when the volume changes, what will be the new pressure?
An ideal gas is enclosed in a constant volume container at a pressure of 0.7atm and an initial temperature of 100°C. The pressure is then decreased to .512atm with a temperature of 37°C. If the pressure is then decreased again to .34atm. What is the final temperature?
A gas under constant pressure has a volume of 30.57m^3 and a temperature of 59.0 K. A change in temperature caused the volume to change to 121.14m^3. Based on the relationship between volume and temperature, what must have happened to the temperature? A- Temperature decreased B- Temperature increased C- Temperature stayed the same D- Temperature trend can not be determined
A hot air balloon uses the principle of buoyancy to create lift. By making the air inside the balloon less dense then the surrounding air, the balloon is able to lift objects many times its own weight. A large hot air balloon has a maximum balloon volume of 2090 m3. a. If the air temperature in the balloon is 54 °C, how much additional mass, in kilograms, can the balloon lift? Assume the molar mass of air is 28.97 g/mol, the air density is 1.20 kg/m3, and the air pressure is 1 atm.
25. A movable circular lid rests on top of an a gas-filled a cylinder; the cylinder and lid have a radius of 12.0 cm; the lid has a weight of 800 N. Outside the cylinder is atmospheric pressure, 1.01 x 105 Pa. Inside the cylinder are 6.0 moles of argon gas. The gas temperature is 400 °K. What is the volume of the gas (in cubic meters)? The atomic mass of argon is 39.95. (a) 0.04 (b) 0.21 (c) 0.17 (d) 0.13 (e) none of these osodilo 0 (0) 2 (0) SC on (s)