What volume in liters (L) of air measured at 1.00 atm would have to be put into a car tire with a volume of 12.9 L, if the pressure in the car tire is to be 32.0 psi? Assume that the temperature of the gas remains constant.

What volume in liters (L) of air measured at 1.00 atm would have to be put into a car tire with a volume of 12.9 L, if the pressure in the car tire is to be 32.0 psi? Assume that the temperature of the gas remains constant.

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter6: The States Of Matter

Section: Chapter Questions

Problem 6.43E

See similar textbooks

Related questions

Q: temperature

A: This question is related to ideal gas equation.

Q: The stopcock connecting a 1.00 L bulb containing neon gas at a pressure of 790. mm Hg, and a 1.00 L…

Q: A sample of argon gas occupies a volume of 6.03 L at 58°C and 446 mm Hg. The volume of the gas…

Q: A certain mass of nitrogen gas occupies a volume of 6.30 L at a pressure of 8.36 atm. At what…

Q: A flexible container at an initial volume of 5.12 L5.12 L contains 3.51 mol3.51 mol of gas. More gas…

A: We can use the formula V1/n1=V2/n2 for solving the problem

Q: A gas cylinder contains 2.45 mol He, 1.85 mol Ne, and 2.15 mol Ar. If the total pressure in the…

Q: If 1.36 g of a gas occupies a volume of 1.00 L at 0.984 atm and 30 C, what is the molar mass in…

A: From ideal gas law, we know that PV = nRT Where P = pressure of the gas V = volume of gas n =…

Q: A gaseous compound is 30.4% nitrogen and 69.6% oxygen by mass. A 5.25g sample of this gas occupies a…

Q: A certain mass of nitrogen gas occupies a volume of 9.64 L at a pressure of 3.59 atm. At what…

Q: ired to decrease the volume of the gas sample to 7.44 L, p 0.540 atm, the temperature of the gas…

A: Initial Volume = 9.40 L Initial Temperature =53 °c = 326 K Initial pressure = 0.440 atm Final…

Q: What is the temperature, in K, of a 1.0 mole sample of gas that initially had a pressure of 1.01…

A: The final pressure in the atm is determined as follows. P2=767.6 torrP2=767.6 torr760 torr/atm=1.01…

Q: An ideal gas is allowed to expand from 8.80 L to 48.4 L at constant temperature. By what factor…

A: Given: An ideal gas is allowed to expand from: V1 = 8.80 L to V2 = 48.4 L at constant…

Q: 2. Equal molar quantities of two gasses of molecular weight 4 and 40 are mixed. The pressure of the…

Q: A sealed flask contains 3.1 L of a gas at 2.4 atm and 22.7 °C. If the density of the gas is 9.7 g/L,…

Q: occupies

A: Ideal gas equation, PV = nRT Temperature is constant PV = constant For, initial condition : P1V1…

Q: Partial pressures The scene below depicts a mixture of four gases. (1) Which gas has the highest…

Q: A sample of hydrogen gas occupies a volume of 8.58 L at 48.0°C and 0.540 atm. If it is desired to…

A: Initial volume (V1) = 8.58 L Initial temperature (T1) = 48.0°C Initial Pressure (P1) = 0.549 atm…

Q: What is the maximum number of balloons that can be inflated? Assume that the gas in the cylinder is…

Q: A gas sample containing 0.6838 moles is trapped in a chamber with a volume of 7.557 liters. If the…

A: n = 0.6838 molV = 7.557 LT = 298.17 K

Q: The ideal gas law allows us to predict that: As the temperature of a gas increases, the volume of…

A: The ideal gas law allows us to predict that: As the temperature of a gas increases, the volume of…

Q: A 0.2L sample of 02 gas has a pressure of 1 atmosphere. If the volume of the 02 gas is decreased to…

A: At constant temperature the amount of gas in a closed container followed the equation: P1V1 = P2V2

Q: If 4.68 g Ar are added to 4.09 atm He in a 2.00 L cylinder at 27.0 °C, what is the total pressure of…

A: no of moles Ar=4.6840 =0.117no of moles of He , under given conditionAssuming…

Q: A sample of oxygen gas occupies a volume of 7.54 L at 49.0°C and 0.940 atm. If it is desired to…

A: Given :- P1 = 0.940 atm V1 = 7.54 L T1 = 49.0°C P2 = 1.17 atm V2 = 6.17 L To calculate :- T2…

Q: The mole fraction of hydrogen gas in a mixture of gases is 0.17. The total pressure of the gas…

A: Partial pressure of a gas can be calculated from the total pressure of the gas mixture if we somehow…

Q: A sample of neon gas occupies a volume of 8.35 L at 44.0°C and 0.960 atm. If it is desired to…

Q: A 16.0 L sample of chlorine gas has a pressure of 28.0 atm at a certain temperature. At the same…

A: According to ideal gas law, PV = nRT where P = pressure V = volume n = moles R = gas constant =…

Q: A 16.0 L sample of argon gas has a pressure of 25.0 atm at a certain temperature. At the same…

Q: What pressure (atm) is needed to confine an ideal gas to 167.0 L after it has expanded from 35.0 L…

A: The ideal gas equation is given as: PV = nRTwhere, P = PressureV = Volumen = Number of moles R =…

Q: A mixture of two gases, A and B, at a total pressure of 2.95 atm is found to contain 0.42 moles of…

A: Given, Total pressure = 2.95 atm Moles of gas A = 0.42 mol Moles of gas B = 0.86 mol Total moles…

Q: A pressurized gas is allowed to expand. If the gas originally occupied a volume of 420 mL at a…

A: Given :- initial pressure = 300 psi Initial volume = 420 mL final…

Q: A certain mass of nitrogen gas occupies a volume of 8.20 L at a pressure of 1.78 atm. At what…

A: The pressure of sample when its volume increases is calculated as,

Q: The stopcock connecting a 1.00 L bulb containing krypton gas at a pressure of 678 mm Hg, and a 1.00…

A: We have to calculate the final pressure

Q: A certain mass of nitrogen gas occupies a volume of 6.63 L6.63 L at a pressure of 6.08 atm.6.08 atm.…

A: According to ideal gas law PV = nRT where P = pressure V = volume n = moles R = gas constant T =…

Q: A certain mass of nitrogen gas occupies a volume of 1.33 L at a pressure of 3.01 atm. At what…

A: A certain mass of nitrogen gas occupies a volume of 1.33 L at a pressure of 3.01 atm. The pressure…

Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

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

Step 2

Step 3

Final answer

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 5 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, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A sample of a compound of xenon and fluorine was confined in a bulb with a pressure of 18 tor. Hydrogen was added to the bulb until the pressure was 72 torr. Passage of an electric spark through the mixture produced Xe and HF. After the HF was removed by reaction with solid KOH, the final pressure of xenon and unreacted hydrogen in the bulb was 36 torr. What is the empirical formula of the xenon fluoride in the original sample? (Note: Xenon fluorides contain only one xenon atom per molecule.)
In an experiment in a general chemistry laboratory, a student collected a sample of a gas over water. The volume of the gas was 265 mL at a pressure of 753 torr and a temperature of 27 C. The mass of the gas was 0.472 g. What was the molar mass of the gas?
As 1 g of (lie radioactive element radium decays over 1 year. k produces 1.161018 alpha particles (helium nuclei). Each alpha particle becomes an atom of helium gas. What is the pressure ¡n pascal of the helium gas produced if it occupies a volume of 125 mL at a temperature of 25 C?
Pressures of gases in mixtures are referred to as partial pressures and are additive. 1.00 L of He gas at 0.75 atm is mixed with 2.00 L of Ne gas at 1.5 atm at a temperature of 25.0 C to make a total volume of 3.00 L of a mixture. Assuming no temperature change and that He and Ne can be approximated as ideal gases, what are a the total resulting pressure, b the partial pressures of each component, and c the mole fractions of each gas in the mix?