Question #20445
1.2g of Silver was roasted in air to form silver 1.289g of silver oxide. Find the Empirical formula for the silver oxide formed.
Expert's answer
Chemical reaction for this process is:
Ag+ x/2 O2= AgxO
If mass of silver = 1.2 and 1.289 is mass of silver oxide, molecular weight of silver oxide is (108x+16)
1.2 & 1.289
Ag+ x/2 O2= AgOx
108 & (108x+16)
108*1.289=1.2*(108+16x)
116.01=108+16x
x=0,5
AgO(0.5) or Ag2O is empirical formula
Ag+ x/2 O2= AgxO
If mass of silver = 1.2 and 1.289 is mass of silver oxide, molecular weight of silver oxide is (108x+16)
1.2 & 1.289
Ag+ x/2 O2= AgOx
108 & (108x+16)
108*1.289=1.2*(108+16x)
116.01=108+16x
x=0,5
AgO(0.5) or Ag2O is empirical formula
