3. at sea level, the atmospheric pressure is 101.3 kpa. atop mount everest, the atmospheric pressure is 33.7 kpa. considering the normal boiling point of water (100 °c) and its heat of vaporization (40.7 kj/mol), at what temperature will water boil atop mount everest? m

Answer : The temperature at top mount everest will be 344 K

Explanation :

The Clausius- Clapeyron equation is :

where,

= atmospheric pressure at at sea level = 101.3 kPa

= atmospheric pressure at top mount everest = 33.7 kPa

= normal boiling point of water =

= temperature at top mount everest = ?

= heat of vaporization = 40.7 kJ/mole = 40700 J/mole

R = universal constant = 8.314 J/K.mole

Now put all the given values in the above formula, we get:

Hence, the temperature at top mount everest will be 344 K

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:

the increase of protons   hope this