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Chapter 5: Problem 86

The boiling point of liquid nitrogen is \(-196^{\circ} \mathrm{C}\). On the basis of this information alone, do you think nitrogen is an ideal gas?

Short Answer

Expert verified
No, nitrogen is not an ideal gas, it is a real gas because it has a boiling point.

Step by step solution

01

Understanding Ideal and Real Gas

Remember, ideal gases are models or theoretical constructs where the gases consist of randomly moving, non-interacting point particles. On the other hand, real gases are actual gases that have interactions between particles and do not always follow the assumptions of the ideal gas model.
02

Analyzing Given Information

In the exercise, it is given that nitrogen has a boiling point of \(-196^{\circ} \mathrm{C}\). Boiling points are a property of real gases, not ideal gases.
03

Making the Conclusion

Since nitrogen has a boiling point, it has properties and behaviors of a real gas. Therefore, nitrogen would not be considered an ideal gas based solely on this information.

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Most popular questions from this chapter

A gas evolved during the fermentation of glucose (wine making) has a volume of \(0.78 \mathrm{~L}\) when measured at \(20.1^{\circ} \mathrm{C}\) and \(1.00 \mathrm{~atm} .\) What was the volume of this gas at the fermentation temperature of \(36.5^{\circ} \mathrm{C}\) and 1.00 atm pressure?

Dissolving \(3.00 \mathrm{~g}\) of an impure sample of calcium carbonate in hydrochloric acid produced \(0.656 \mathrm{~L}\) of carbon dioxide (measured at \(20.0^{\circ} \mathrm{C}\) and \(792 \mathrm{mmHg}\) ). Calculate the percent by mass of calcium carbonate in the sample. State any assumptions.

A sample of zinc metal is allowed to react completely with an excess of hydrochloric acid: $$\mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g)$$ The hydrogen gas produced is collected over water at \(25.0^{\circ} \mathrm{C}\) using an arrangement similar to that shown in Figure \(5.14 .\) The volume of the gas is \(7.80 \mathrm{~L},\) and the atmospheric pressure is \(0.980 \mathrm{~atm} .\) Calculate the amount of zinc metal in grams consumed in the reaction. (Vapor pressure of water at \(25^{\circ} \mathrm{C}=\) \(23.8 \mathrm{mmHg} .)\)

What does the Maxwell speed distribution curve tell us? Does Maxwell's theory work for a sample of 200 molecules? Explain.

Why is mercury a more suitable substance to use i a barometer than water?
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