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Chapter 1: Problem 12

Identical amounts of the four gases listed below are present in four separate balloons. At STP, which balloon size experiences the greatest deviation from the volume calculated using the Ideal Gas Law? $\begin{array}{ll}{\text { (A) }} & {\mathrm{H}_{2}} \\ {\text { (B) }} & {\mathrm{O}_{2}} \\ {\text { (C) }} & {\mathrm{N}_{2}} \\ {\text { (D) }} & {\mathrm{F}_{2}}\end{array}$

Short Answer

Expert verified
The balloon with Fluorine gas (F2) would experience the greatest deviation from the Ideal Gas Law because it has the highest molecular mass and strongest intermolecular forces amongst the listed gases.

Step by step solution

01

Step 1. Identify the molecular masses

In this step, identify the molecular masses of the gases presented. These are Hydrogen (H2), Oxygen (O2), Nitrogen (N2), and Fluorine (F2). The molecular masses are approximately 2, 32, 28, and 38 g/mol respectively.
02

Step 2. Identify the intermolecular forces

Consider the types of intermolecular forces that each of these gases possess. Hydrogen (H2), Oxygen (O2), Nitrogen (N2) gases consists predominantly of London dispersion forces, while Fluorine (F2) has strong intermolecular forces due to its high electronegativity and polarizability.
03

Step 3. Correlate molecular mass and intermolecular forces with deviations from Ideal Gas Law

Gases with high molecular masses and strong intermolecular forces show the greatest deviation from Ideal Gas Law because their particles don't have zero volume and they experience significant attractions or repulsions. Therefore, the gas with the highest molecular mass and strongest intermolecular force, which is F2, will show the greatest deviation from the volume predicted under the Ideal Gas Law.

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Most popular questions from this chapter

\(\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{2} \mathrm{O}(s)\) Which of the following is true for the above reaction? (A) The value for \(\Delta S\) is positive. (B) The value for \(\Delta G\) is zero. (C) The value for \(\Delta H\) is positive. (D) The reaction is favored at 1.0 \(\mathrm{atm}\) and 298 \(\mathrm{K}\) .

For a reaction involving nitrogen monoxide inside a sealed flask, the value for the reaction quotient \((Q)\) was found to be \(1.1 \times 10^{2}\) at a given point. If, after this point, the amount of NO gas in the flask increased, which reaction is most likely taking place in the flask? (A) \(\operatorname{NOBr}(g) \rightarrow \operatorname{NO}(g)+1 / \operatorname{Br}_{2}(g) \quad K_{\mathrm{C}}=3.4 \times 10^{-2}\) (B) \(2 \mathrm{NOCl}(g) \mapsto 2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \quad K_{\mathrm{c}}=1.6 \times 10^{-5}\) (C) \(2 \mathrm{NO}(g)+2 \mathrm{H}_{2}(g) \rightarrow \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g) \quad K_{\mathrm{c}}=4.0 \times 10^{6}\) (D) \(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{NO}(g) \quad K_{\mathrm{c}}=4.2 \times 10^{2}\)

\(\begin{array}{ll}{\mathrm{Cu}^{2+}+2 e^{-} \rightarrow \mathrm{Cu}} & {E^{\circ}=+0.3 \mathrm{V}} \\ {\mathrm{Zn}^{2+}+2 e^{-} \rightarrow \mathrm{Zn}} & {E^{\circ}=-0.8 \mathrm{V}} \\ {\mathrm{Mn}^{2+}+2 e^{-} \rightarrow \mathrm{Mn}} & {E^{\circ}=-1.2 \mathrm{V}}\end{array}\) Based on the reduction potentials given above, which of the following reactions will be favored? (A) \(\mathrm{Mn}^{2+}+\mathrm{Cu} \rightarrow \mathrm{Mn}+\mathrm{Cu}^{2+}\) (B) \(\mathrm{Mn}^{2+}+\mathrm{Zn} \rightarrow \mathrm{Mn}+\mathrm{Zn}^{2+}\) (C) \(\mathrm{Zn}^{2+}+\mathrm{Cu} \rightarrow \mathrm{Zn}+\mathrm{Cu}^{2+}\) (D) \(\mathrm{Zn}^{2+}+\mathrm{Mn} \rightarrow \mathrm{Zn}+\mathrm{Mn}^{2+}\)

150 \(\mathrm{mL}\) of saturated \(\mathrm{SrF}_{2}\) solution is present in a 250 \(\mathrm{mL}\) beaker at room temperature. The molar solubility of \(\mathrm{SrF}_{2}\) at 298 \(\mathrm{K}\) is \(1.0 \times 10^{-3} \mathrm{M}\) . If some of the solution evaporates overnight, which of the following will occur? (A) The mass of the solid and the concentration of the ions will stay the same. (B) The mass of the solid and the concentration of the ions will increase. (C) The mass of the solid will decrease, and the concentration of the ions will stay the same. (D) The mass of the solid will increase, and the concentration of the ions will stay the same.

$$4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \rightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)$$ The above reaction will experience a rate increase by the addition of a catalyst such as platinum. Which of the following best explains why? (A) The catalyst causes the value for \(\Delta G\) to become more negative. (B) The catalyst increases the percentage of collisions that occur at the proper orientation in the reactant molecules. (C) The catalyst introduces a new reaction mechanism for the reaction. (D) The catalyst increases the activation energy for the reaction.
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