**Question:**Calculate the ratio of the effusion rates of helium gas (He) and uranium hexafluoride (UF₆), a gas used in the enrichment process to produce fuel for nuclear reactors.**Options:**- ○ 87.9- ○ 13.2- ○ 9.38- ○ None of these- ○ 352.02**Explanation:**To solve this problem, you would use Graham's Law of Effusion, which states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. The formula to calculate the ratio of effusion rates is:\[ \frac{\text{Rate of effusion of He}}{\text{Rate of effusion of UF₆}} = \sqrt{\frac{\text{Molar mass of UF₆}}{\text{Molar mass of He}}} \]The ratio will help determine how much faster helium effuses compared to uranium hexafluoride. Calculating this involves using the known molar masses of helium and UF₆. The image contains a graph and multiple-choice question related to the behavior of Nitrogen gas under different conditions.**Graph Description:**- The graph is a plot of \( \frac{PV}{nRT} \) (y-axis) against pressure \( P \) in atm (x-axis). - There are three colored curves each representing a different temperature: 203 K (green), 293 K (purple), and 673 K (orange).- A dashed horizontal line at \( \frac{PV}{nRT} = 1.0 \) indicates ideal gas behavior.- The curve for 673 K (orange) is almost flat and close to the ideal line, indicating behavior closer to an ideal gas at that temperature.- The 203 K (green) and 293 K (purple) curves deviate more from the ideal line, especially as pressure increases.**Question:**"What does this graph represent for Nitrogen?"**Answer Options:**- None of these is true- This graph shows that Nitrogen gas behaves most ideally at higher temperature and lower pressure- This graph shows that Nitrogen at no point behaves anywhere close to being ideal.- This graph shows that Nitrogen gas behaves ideally at lower temperature and higher pressure.- This graph shows that Nitrogen gas behaves more ideally at lower temperature and lower pressure.

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Calculate the ratio of the effusion rates of helium gas (He) and uranium hexafluoride (UF6), a gas used in the enrichment process to produce fuel for nuclear reactors 87.9 | 13.2 9.38 None of these 352.02

Calculate the ratio of the effusion rates of helium gas (He) and uranium hexafluoride (UF6), a gas used in the enrichment process to produce fuel for nuclear reactors 87.9 | 13.2 9.38 None of these 352.02

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.

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