The atomic mass number of aluminum is 26.98. If you had 1.34 x 1025 atoms of aluminum, how much would they all weigh? 3.62 grams
601 grams
3.62 x 1026 grams
1.21 grams

601 gram

Explanation:

1st we should know how may moles are there in 1.34 X 10 25 atoms

 # moles of Al = # of atoms / # of Avogadro's num

                      = 1.34 X 10 25/ 6.12X10 23 =

                       = 22.26 mol of AL

 so mass of AL = moles x m.wt

                          =22.26 x 26.98 = 600.55 = 601 gram

DONE

oh it is true if thats what you are asking

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