A gas is contained in a cylinder With the volume of 5.4 L at a temperature of 32.5°C in a pressure of 673.2 torr. The gas is then compressed to a volume of 0.13 L and the temperature is right to 520.5°C. What is the new pressure of the gas ?

The new pressure of the gas is 95.54 atm or 72610 torr

Explanation:

Step 1: Data given

Volume of the cylinder = 5.4 L

The initial temperature = 32.5 °C = 305.65 K

The initial pressure = 673.2 torr = 0.88578947 atm

The volume decreases to 0.13 L

The temperature is increased to 520.5 °C = 793.65 K

Step 2: Calculate the new pressure

P1*V1 / T1   = P2*V2/T2

⇒with P1 = the initial pressure =673.2 torr = 0.88578947 atm

⇒with V1 = the initial volume = 5.4 L

⇒with T1 = the initial temperature = 32.5 °C = 305.65 K

⇒with P2 = the final pressure = TO BE DETERMINED

⇒with V2 = the final volume = 0.13 L

⇒with T2 = the final temperature = 793.65 K

0.88578947 atm *5.4 / 305.65 = P2 * 0.13 / 793.65

P2 = 95.54 atm = 72610 torr

The new pressure of the gas is 95.54 atm or 72610 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: