Imagine that you have a 5.00 L gas tank and a 2.00 L gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 136 bar , to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behaviour for all gases.

Imagine that you have a 5.00 L gas tank and a 2.00 L gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 136 bar , to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behaviour for all gases.

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter1: Gases And The Zeroth Law Of Thermodynamics

Section: Chapter Questions

Problem 1.32E

See similar textbooks

Similar questions

Numerically evaluate for one mole of methane acting as a van der Waals gas at a T = 298 K and V = 25.0 L and b T = 1000 K and V = 250.0 L. Comment on which set of conditions yields a number closer to that predicted by the ideal gas law. pVT,n
Under what conditions of temperature does a Redlich-Kwong gas behave like an ideal gas? Use the Redlich-Kwong equation of state to justify your answer.
Use the ideal gas law to demonstrate the cyclic rule of partial derivatives.
At the critical point for carbon dioxide, the substance is very far from being an ideal gas. Prove this statement by calculating the density of an ideal gas in g/cm3 at the conditions of the critical point and comparing it with the experimental value. Compute the experimental value from the fact that a mole of CO2 at its critical point occupies 94 cm3.
The atmospheric surface pressure on Venus is 90 bar and is composed of 96 carbon dioxide and approximately 4 various other gases. Given a surface temperature of 730 K, what is the mass of carbon dioxide present per cubic centimeter at the surface?
A hot-air balloon achieves its buoyant lift by heating the airinside the balloon, which makes it less dense than the air outside.Suppose the volume of a balloon is 1800 m3 and therequired lift is 2700 N (rough estimate of the weight of theequiptment and passenger). Calculate the temperature of the airinside the balloon which will produce the required lift. Assumethat the outside air temperature is 0 degrees C and that the air isan ideal gas under these conditions.How do I go about applying the ideal gas law to a problem like thiswhich asks me to factor in buoyant lift?Thanks!
The pressure of the gas inside an aerosol can is 1.2 bar at a temperature of25 oC. Will the aerosol explode if it is thrown into a fire and heated to atemperature of 600 oC? Assume that the aerosol can is unable to withstandpressures in excess of 3 bar.
Gases - Please answer all components of this problem; Thank you! 1. Explain how ideal and real gases are similar and different. Is it possible for a real gas to behave ideally? If so, please describe how this would be possible.
The gas A(g) (1 mole) undergoes a two-step process one after another as described below :i) The gas is expanded at 25°C and from 1 bar pressure against a constant pressure of 0.2 bar and the final volume of the gas is the twice the initial volume.ii) The gas is cooled down to -25°C at constant volume.Cv,m = 3/2 RCalculate ΔU, ΔH, q and w for the each step and for the entire process
What Is The Ideal-Gas Equation of State?
The ammonia contained in a container measuring rectangular tank 1m x 700 cm x 3000mm if the pressure is 1.5 bar and temperature is 28 0C. Assume the molecular weight ofammonia is 17. Calculate the mass of ammonia
An ideal gas confined to a container with a massless piston at the top. A massless wire is attacted to the piston. When an external pressure of 2.00 atm is applied to the wire, the gas compresses from 4.90 to 2.45L. When the external pressure is increased to 2.50 atm, the gas futher compresses from 2.45 to 1.96L In a seperate experiment with the same initial conditions of 2.50 atm was applied to the ideal gas, decreasing its volume from 4.90 to 1.96L in one step. If the final temperture was the same for both processes, what is the difference between q for the two step pocess and q for the one process in joules?