What mass of oxygen forms from 71.89 g CO2?
Use the periodic table to find molar masses.
71.89 g CO2 =
gO₂
rom
DONE
2.18

Explanation:

1. Molar masses

(a) CO₂

1 C =  1 ×  12.01 u =  12.01 u

2 O = 2 × 16.00 u = 32.00 u

                 TOTAL = 44.01 u

(b) O₂

2 O = 2 × 16.00 u = 32.00 u

2. Mass of oxygen produced

We will need a chemical equation with masses and molar masses, so, let's gather all the information in one place.

Mᵣ:    44.01         32.00

         CO₂ ⟶ C + O₂

m/g:  71.89

So, 32.00 g of oxygen form from 44.01 g of CO₂  

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