5. 4.50 moles of a certain gas occupies a volume of 550.0 mL at 5.000ºC and 1.000 atm. What would the volume be if 10.50 moles are present at 27.00°C and 1.250 atm? HELPPP

The final volume is 1108 ml

Explanation:

According to combined gas law:

Where :

= initial pressure = 1.000 atm

= initial volume = 550.0 ml

= initial moles = 4.50

= initial temperature =

= final pressure = 1.250 atm

= final volume = ?

= final moles = 10.50

= final temperature =

Thus final volume is 1108 ml

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:

i think its 100

i hope this !