what is the mass of 6.02 x 1023 atoms of sulfur?
a. 6.02 x 1023 g
b. (6.02 x1029) g
32
c. 32(6.02 x 1023) g
d. 32g

32 g

Explanation:

molar masses of elements such as sulfur can be found on the periodic table.

the molar mass listed on the periodic table equals 1 mole of the atom which also equals 6.02×10^23

therefore, 32g = 1 mole of sulfur = 6.02×10^23

(1 mole always equals 6.02×10^23)

there are no statements provided but here is why:

sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

hope this

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml