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Chapter 9: Q42E (page 509)

A litre of methane gas, \({\rm{C}}{{\rm{H}}_4}\), at STP contains more atoms of hydrogen than does a litre of pure hydrogen gas, \({{\rm{H}}_2}\), at STP. Using Avogadro's law as a starting point, explain why.

Short Answer

Expert verified

Therefore, a litre of methane gas at STP contains more atoms of hydrogens than does a litre of pure hydrogen gas.

Step by step solution

01

Step 1: Avogadro's law

Avogadro's law asserts that equal volumes of various gases contain an equal number of molecules at the same temperature and pressure.

02

Explanation

The number of Avogadro's molecules in one litre of methane gas and one litre of pure hydrogen gas at STP is the same.

However, one methane molecule has four hydrogen atoms, whereas the hydrogen gas has two hydrogen atoms.

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Most popular questions from this chapter

Question: Show that the ratio of the rate of diffusion of Gas1to the rate of diffusion of Gas 2, \(\frac{{{{\rm{R}}_{\rm{1}}}}}{{{{\rm{R}}_{\rm{2}}}}}\), is the same at 00C and 1000C.

Calculate the density of Freon \(12,{\rm{C}}{{\rm{F}}_2}{\rm{C}}{{\rm{l}}_2}\), at \({30.0^\circ }{\rm{C}}\) and \(0.954\;{\rm{atm}}\).

Consider this question: What is the molecular formula of a compound that contains \(39\% {\rm{C}}\,\,,45\% \;{\rm{N}}\), and \(16\% \,{\rm{H}}\) if \(0.157\;{\rm{g}}\)of the compound occupies \(125\;{\rm{mL}}\) with a pressure of \(99.5{\rm{kPa}}\)at \({22^\circ }{\rm{C}}\)?

(a) Outline the steps necessary to answer the question;

(b) Answer the question.

Question: Answer the following questions:

(a) If \({\rm{XX}}\) behaved as an ideal gas, what would its graph of \({\rm{Z}}\) vs. \({\rm{P}}\) look like?

(b) For most of this chapter, we performed calculations treating gases as ideal. Was this justified?

(c) What is the effect of the volume of gas molecules on \({\rm{Z}}\)? Under what conditions is this effect small? When is it large? Explain using an appropriate diagram.

(d) What is the effect of intermolecular attractions on the value of \({\rm{Z}}\)? Under what conditions is this effect small? When is it large? Explain using an appropriate diagram.

(e) In general, under what temperature conditions would you expect \({\rm{Z}}\) to have the largest deviations from the \({\rm{Z}}\) for an ideal gas?

How would the graph in Figure \({\rm{9}}{\rm{.13}}\) change if the number of moles of gas in the sample used to determine the curve were doubled?
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