Which exhibits the most ideal behavior at stp

Asked 4 years, 8 months ago. Active 4 years, 8 months ago. Viewed 1k times. I sort of don't agree with this logic. Let us have a look at Andrew's curves: We notice that greater is the temperature compared to critical temperature more is the ideal behaviour. Improve this question. Community Bot 1. But the bigger problem is he said that difference between Tc and should be minimum for ideal behavior. Shouldn't it be maximum for ideal behavior? Air pollution contributes to poor health through respiratory conditions, heart disease, and lung cancer.

Approximately 3. Free radicals in the upper stratosphere act as catalysts for ozone decomposition, thereby depleting the ozone layer. The latter phenomenon is referred to as the ozone hole. Both types of ozone depletion have increased as emissions of halo-carbons have increased. Largest ozone hole observed : In September, , the average area of the ozone hole, displayed here in purple, was The most important process in hole formation is the catalytic destruction of ozone by atomic halogens.

The main source of these halogen atoms in the stratosphere is photodissociation of man-made halocarbon refrigerants; examples include CFCs chlorofluorocarbons , freons, and halons. The Montreal Protocol bans the production of ozone-depleting chemicals such as carbon tetrachloride and trichloroethane. The largest ozone hole was observed in September, In the stratosphere, absorption of ultraviolet photons results in the photodissociation breaking apart of oxygen molecules.

The balanced equation for this reaction is:. The reaction of these free radicals with ozone disrupts the ozone-oxygen cycle, leading to the destruction of stratospheric ozone and the depletion of the ozone layer.

The atomic chlorine and bromine radicals are found in certain stable organic compounds, especially CFCs, which can make their way to the stratosphere because of their low reactivity. Once in the stratosphere, ultraviolet light liberates the Cl and Br atoms from their parent compounds:. The Cl and Br atoms can then destroy ozone molecules through a variety of catalytic cycles. In the simplest example of such a cycle, a chlorine atom reacts with an ozone molecule, taking an oxygen atom forming ClO, chlorine monoxide and leaving a normal oxygen molecule O 2.

The chlorine monoxide can then react with a second molecule of ozone O 3 to yield another chlorine atom and two molecules of oxygen. The chemical equations for these gas-phase reactions are:.

Thus, the atomic chlorine radical regenerates; a single chlorine can keep destroying ozone acting as a catalyst for up to two years. The overall effect is a decrease in the amount of ozone, though null cycles can decrease the rate of these processes. More complicated mechanisms that lead to ozone destruction in the lower stratosphere have also been been discovered.

A common misconception is that because CFC molecules are heavier than air both nitrogen and oxygen , they cannot reach the stratosphere in significant amounts and therefore do not contribute significantly to ozone depletion. Atmospheric gases are not sorted by weight, however; wind forces can fully mix the gases in the atmosphere, which readily diffuse into the stratosphere.

Privacy Policy. Skip to main content. Search for:. Deviation of Gas from Ideal Behavior The Effect of the Finite Volume Real gases deviate from the ideal gas law due to the finite volume occupied by individual gas particles.

Learning Objectives Demonstrate an understanding of the van der Waals equation for non-ideal gases. Key Takeaways Key Points The ideal gas law assumes that gases are composed of point masses that interact via completely elastic collisions. Real gases are made up of particles that occupy a non-zero volume known as the excluded volume. Skip to content Chapter 9. Learning Objectives By the end of this section, you will be able to: Describe the physical factors that lead to deviations from ideal gas behavior Explain how these factors are represented in the van der Waals equation Define compressibility Z and describe how its variation with pressure reflects non-ideal behavior Quantify non-ideal behavior by comparing computations of gas properties using the ideal gas law and the van der Waals equation.

Calculate the pressure of this sample of CO 2 : a from the ideal gas law b from the van der Waals equation c Explain the reason s for the difference. Answer: a Chemistry End of Chapter Exercises Graphs showing the behavior of several different gases follow.

Which of these gases exhibit behavior significantly different from that expected for ideal gases? Explain why the plot of PV for CO 2 differs from that of an ideal gas.

Under which of the following sets of conditions does a real gas behave most like an ideal gas, and for which conditions is a real gas expected to deviate from ideal behavior? Calculate the pressure: a using the ideal gas law b using the van der Waals equation c Explain the reason for the difference. Answer the following questions: a If XX behaved as an ideal gas, what would its graph of Z vs.

Glossary compressibility factor Z ratio of the experimentally measured molar volume for a gas to its molar volume as computed from the ideal gas equation van der Waals equation modified version of the ideal gas equation containing additional terms to account for non-ideal gas behavior. Solutions 1. Gases C, E, and F 3. Previous: 9. Next: Introduction.

Share This Book Share on Twitter. In his description of gas behavior, the so-called van der Waals equation,. The volume term corrects for the volume occupied by the gaseous molecules. The correction for volume is negative, but the correction for pressure is positive to reflect the effect of each factor on V and P , respectively.

Because nonzero molecular volumes produce a measured volume that is larger than that predicted by the ideal gas law, we must subtract the molecular volumes to obtain the actual volume available. You are in charge of the manufacture of cylinders of compressed gas at a small company.

Your company president would like to offer a 4. The cylinders you have on hand have a rupture pressure of 40 atm. Is this cylinder likely to be safe against sudden rupture which would be disastrous and certainly result in lawsuits because chlorine gas is highly toxic? Given: volume of cylinder, mass of compound, pressure, and temperature. A Use the molar mass of chlorine to calculate the amount of chlorine in the cylinder. Then calculate the pressure of the gas using the ideal gas law.

Based on the value obtained, predict whether the cylinder is likely to be safe against sudden rupture. A We begin by calculating the amount of chlorine in the cylinder using the molar mass of chlorine Using the ideal gas law and the temperature in kelvin K , we calculate the pressure:. This pressure is well within the safety limits of the cylinder.