Answer:
b. Specific heat increases as the number of atoms per molecule increases.
c. Specific heat at constant pressure is higher than at constant volume.
d. Monatomic gases behave like ideal gases.
Explanation:
Specific heat of the gas at constant pressure is usually higher than that of the volume.
i.e.
Cp - Cv = R
where R is usually the gas constant.
However, monoatomic gases are gases that exhibit the behavior of ideal gases. This is due to the attribute of the intermolecular forces which plays a negligible role. Nonetheless, the case is not always true for all temperatures and pressure.
Similarly, the increase in the number of atoms per molecule usually brings about an increase in specific heat. This effect is true as a result of an increase in the total number associated with the degree of freedom from which energy can be separated.
Thus, from above explanation:
Option b,c,d are correct while option (a) is incorrect.
Newton's Laws<span>. </span>Kepler's Laws<span> are wonderful as a description of the </span>motions<span> of the </span>planets<span>. However, they provide no explanation of why the </span>planets<span> move in this way. Moreover, </span>Kepler's<span> Third </span>Law<span> only works for </span>planets<span> around the Sun and does not apply to the Moon's orbit around the Earth or the moons of Jupiter.
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When energetic UV rays dissociates molecules of oxygen into seperate atoms. But when they collide into each other it forms OZONE.
