A 35.0 L sample of gas collected in the upper atmosphere at a pressure of 48.6 torr is compressed into a 150. mL container at constant temperature. What is the new pressure (atm)? (4pts) 1 atm = 760 torr

The new pressure (atm) = 14.7 atm or 11172 torr

Explanation:

                                 P₁V₁ = P₂V₂ (using Boyle's law at constant temperature)

Volume of sample of gas collected in the upper atmosphere (V₁) = 35.0 Lit

pressure of the gas (P₁) = 48.6 torr

                           1 atm = 760 torr

                     ⇒    

                     ⇒   48.6 torr = 48.6 x 0.00131 = 0.063 atm

Volume after compression (V₂) = 150 ml = 0.15 lit

  New pressure (P₂) = ?

                                          P₁V₁ = P₂V₂

                          ⇒          P₂ =

                          ⇒         P₂ = or 11172 torr            

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: