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Chapter 1: Problem 6

State whether the following statements are true or false. Gases show deviations from ideal behaviour at high temperatures and high pressures.

Short Answer

Expert verified
Based on the analysis of the ideal gas law and the conditions under which gases exhibit ideal behavior, is the following statement TRUE or FALSE: "Gases show deviations from ideal behavior at high temperatures and high pressures." Answer: FALSE

Step by step solution

01

Understand the ideal gas law

The ideal gas law is represented by the equation PV = nRT, where P is the pressure of the gas, V is the volume, n represents the number of moles, R is the ideal gas constant, and T is the temperature. This equation is valid for an ideal gas, which is a hypothetical gas that obeys the ideal gas law perfectly under all conditions.
02

Recognize conditions for ideal gas behavior

Real gases can approximate ideal behavior under certain conditions, specifically low pressures and high temperatures. Low pressures provide enough space between gas particles for the intermolecular forces to become negligible, while high temperatures allow gas particles to move at higher velocities and their kinetic energies to dominate over intermolecular forces.
03

Analyze the statement about deviations from ideal behavior

Now we can examine the given statement: "Gases show deviations from ideal behavior at high temperatures and high pressures." We've established that gases closely follow ideal behavior at high temperatures and low pressures. However, the statement claims that gases deviate from ideal behavior at high temperatures and high pressures.
04

Determine the validity of the statement

Since we know that gases are more likely to follow ideal behavior when they are at high temperatures and low pressures, the statement which claims that gases deviate from ideal behavior at high temperatures and high pressures is FALSE. The correct statement should say "Gases show deviations from ideal behavior at low temperatures and high pressures," which is when real gases exhibit more significant deviations from ideal behavior due to more substantial intermolecular forces and reduced kinetic energies.

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Most popular questions from this chapter

Match the entries given in Column A with appropriate ones in Column \(B\). $$ \begin{array}{|l|l|l|} \hline \begin{array}{l} \text { A. Empirical formula of } \\ \text { glucose } \end{array} & \text { () } & \begin{array}{l} \text { a. Less intermolecular } \\ \text { forces } \end{array} \\ \hline \begin{array}{l} \text { B. Percentage of carbon } \\ \text { in methane } \end{array} & \text { () } & \text { b. } 75 \% \\ \hline \text { C. Ideal gas } & \text { () } & \text { c. } 17.6 \% \\ \hline \text { D. High critical } & \text { () } & \begin{array}{l} \text { d. } \text { Large } \\ \text { intermolecular } \\ \text { forces of attraction } \end{array} \\ \hline \begin{array}{l} \text { E. Percentage of } \\ \text { hydrogen in } \\ \text { ammonia } \end{array} & \text { () } & \text { e. } \mathrm{CH}_{2} \mathrm{O} \\ \hline \begin{array}{l} \text { F. } \text { Empirical formula of } \\ \text { oxalic acid } \end{array} & \text { () } & \text { f. } \mathrm{CHO}_{2} \\ \hline \end{array} $$

The number of oxygen atoms present in 2 moles of a compound, which consists of a bivalent metal and a perchlorate ion is (a) \(4 \mathrm{~N}\) (b) \(6 \mathrm{~N}\) (c) \(8 \mathrm{~N}\) (d) \(16 \mathrm{~N}\)

\(23 \mathrm{~g}\) of \(\mathrm{NO}_{2}\) contains same number of molecules as (a) \(8 \mathrm{~g}\) of oxygen (b) \(28 \mathrm{~g}\) of carbon monoxide (c) \(16 \mathrm{~g}\) of \(\mathrm{SO}_{2}\) (d) \(22 \mathrm{~g}\) of \(\mathrm{CO}_{2}\)

State whether the following statements are true or false. The greater the critical temperature of a gas, the easier is the liquefaction of the gas.

Select the correct alternative from the given choices. \(20 \mathrm{cc}\) of a hydrocarbon on complete combustion gave \(80 \mathrm{cc}\) of \(\mathrm{CO}_{2}\) and \(100 \mathrm{cc}\) of \(\mathrm{H}_{2} \mathrm{O}\) at \(\mathrm{STP}\). The empirical formula of that compound is (a) \(\mathrm{C}_{2} \mathrm{H}_{5}\) (b) \(\mathrm{C}_{2} \mathrm{H}_{6}\) (c) \(\mathrm{C}_{3} \mathrm{H}_{8}\) (d) \(\mathrm{C}_{4} \mathrm{H}_{10}\)
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