For real gases, how does a change in pressure affect the ratio of pvto nrt?
a. the ratio increases as pressure increases.
b. the ratio is constant at all pressures.
c. the ratio decreases as pressure increases.

Explanation:

You can deduce the ratio of PV to nRT from the ideal gas equation.

        ⇒ PV / nRT = 1.

Thus the ratio PV to nRT is constant and equal to 1, at all pressures, such as the statement B describes.

Hence, if P increases or decreases, the other variables, V, n, or T must change to keep the ration constant and equal to 1. R is the universal constant.

The correct answer option is A. the ratio increases as the pressure increases.

Explanation:

We are to determine whether which of the given answer options explains how does a change in pressure affect the ration of PV to nRT.

We know that, for real gases:

where,

is the pressure of the gas ,

is the volume of gas ,

is the number of moles ,

is the gas constant; and

 is the temperature of the gas.

Gay-Lussac’s law states that for a constant volume, the pressure of that gas is directly proportional to the temperature on the Kelvin scale.

Therefore, the ratio increases as the pressure increases.

the grams   of   barium that   are in   2.3 x 10^23   atoms of barium   is   52.4 g (answer c)

    calculation

mass = moles   of ba   x molar   mass of ba

  molar mass of ba from periodic table=   137.3 g/mol

  use the   avogadro's law   constant   to   calculate the moles of barium

  that   is     1 mole =   6.02   x 10^23 atoms

                    ? moles = 2.3 x 10^23   atoms

by cross   multiplication

=(1 mole   x 2.3x 10^23 atoms)   / 6.02   x10^23 atoms)=   0.382   moles

mass   is therefore = 137.3   g/mol x 0.382 mol = 52.4 ( answer c)

explanation: