Consider the equations below. CH,(9) →C(s)+2H2 (9) AH, = 74.6 kJ
C(s) + 2Cl2(g) → CCI (9) AH2 = -95.7 kJ
2H2(g) + 2Cl2(g) → 4HCI(9) AH2 = -184.6 kJ
CH, (g) + 4C12(g) → CCI,(9) + 4HCl(g) AH, = -205.7 kJ
Complete the following based on the diagram.
Arrow A:
Arrow B:
Arrow C:
Arrow D:

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:

it is a solid

explanation:

it is stable as it is in group 0 which have full outer shells of electrons