Question

Which of the following best explains why the two values in Parts A and B are different? The perceived forces between chlorine gas molecules that contribute to nonideal behavior are most strongly influenced by Which of the following best explains why the two values in Parts A and B are different? the high system pressure and relatively large chlorine molecule size. the polar chlorine molecules and the low system temperature. the high system temperature and relatively large chlorine molecule size. the high system pressure and high system temperature.

Answer 1

Step-by-step explanation:

According to the Ideal Gas Equation, the pressure generated by a gas is defined as:

P= nRT / V

For non-ideal behaviour, the pressure is represented as:

P=[nRT / V-nb]-n^2a / V^2

The second formula takes into consideration the inter-molecular attraction forces between gas molecules that correspond to its non-ideal behavior. High pressures, low temperatures and relatively large size of the gas molecule are the conditions which strongly influence non-ideal behavior.

The gas molecules are in a space where they are closer together at high pressures and hence the effect of the inter-molecular forces is important.

The kinetic energy of the gas molecules also decreases at low temperatures along with it the energy required to resolve the inter-molecular attraction forces will decrease.

Large size indicates higher atomic number and thus more electrons. The electron cloud surrounding a gas molecule will produce an induced dipole creating interactions between the dipole and the dipole.

The high system pressure and the genuinely large amount of chlorine will lead to the non-ideal behavior from the given choices.

Answer 2

The high system pressure and relatively large chlorine molecule size.

Step-by-step explanation:

Having the expression of the ideal gas, and clearing the pressure, we have:

P = nRT/V

Meanwhile, for a non-ideal gas we have the following equation:

P = (nRT / V-nb) - n2a/V2

In this equation, high pressures and low temperatures have an influence on nonideal gases.

Therefore, at high pressures, the molecules in a gas are closer together and have high intermolecular forces. On the other hand, at low temperatures, the kinetic energy of a gas is reduced, so that the intermolecular attractive forces are also reduced.