Which of the following best helps explain why the pressure of a sample of CH4(g) (molar mass 16g/mol) is closer to the pressure predicted by the ideal gas law than a sample of NH3(g) (molar mass 17g/mol) ?NH3 molecules are polar while CH4 molecules are not, and the greater attractions between NH3 molecules cause the molecules to collide with the walls of the container with less force.

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10-12-2022
Chemistry

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Which of the following best helps explain why the pressure of a sample of CH4(g) (molar mass 16g/mol) is closer to the pressure predicted by the ideal gas law than a sample of NH3(g) (molar mass 17g/mol) ?NH3 molecules are polar while CH4 molecules are not, and the greater attractions between NH3 molecules cause the molecules to collide with the walls of the container with less force.

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AmitPaswan AmitPaswan · Answer 1 · 2022-12-14T15:02:37+01:00

The following best helps to explain that the pressure of a sample of CH₄ is closer to the pressure predicted by gas law than a sample of NH₃ is NH₃ molecules are polar while CH₄ molecules are not.

The methane mole , CH₄ is the non polar molecule. the bond present between the CH₄ is the covalent bond. the compound is called as the covalent compound. the covalent compound is formed by the sharing of the electron pairs. The NH₃ is polar molecule. the NH₃ is also form the covalent bond but it has net dipole moment so, NH₃ is the polar covalent bond.

Thus, the pressure of a sample of CH₄ (molar mass 16g/mol) is closer to the pressure by the ideal gas law than a sample of NH₃ (molar mass 17g/mol): NH₃ molecules are polar while CH₄ molecules are not.

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