What mass of oxygen forms from 71.89 g co2? use the periodic table to find molar masses. 71.89 g co2 = g o2

Atomic mass C = 12.0107
Atomic mass O= 15.9994
Calculate the molecular mass of the CO2
12.0107 + (2 x 15.9994) = 44.0095

Multiply the mass of CO2 by the conversion factor that relate the O mass to the molecular mass of CO2 to find the mass of O in the 71.89g of CO2

71.89 g CO2 x (2 x 15.9994) / 44.0095 =

52.2703900748702

52.27 g O

m=9

step-by-step explanation:

7m+8=71 subtract   8 from 71 which is 63 than divide it by 7m   equal 9.

                             

Since there is the same amount of agn03 in both silver chloride and silver nitrate they produce the same amount of moles. therefore silver chloride produces the same amount of silver nitrate, so your answer is 15.0 moles of silver nitrate. i hope this !