Nitrogen and oxygen extensive series of oxides with the general formula NxOx. One of them is a blue solid that comes apart, reversibly, in the gas phase. It contains 36.84% N. What is the empirical formula of this oxide?
Answers
Answer:
N2O3
Explanation:
Work out the number of moles in
100.00
grams of the oxide.
For nitrogen: The atomic mass of
N
is
14.0067
, and we have
36.84
g N
:
36.84
g N
14.0067
g N/mol N
=
2.630
mol N
For oxygen: The atomic mass of
O
is
15.9994
, and we have
100.00
−
36.84
=
63.16
g O
:
63.16
g N
15.9994
g N/mol N
=
3.948
mol N
Now the ratio
3.958
2.630
is very close to
1.5
=
3
2
. So we conclude that the gas has three moles
O
to two moles
N
making the empirical formula
N
2
O
3
.
Answer:
Work out the number of moles in 100.00 grams of the oxide.
For nitrogen: The atomic mass of N is 14.0067 , and we have 36.84 g N :
36.84 g N /14.0067 g N/mol N = 2.630 mol N
For oxygen: The atomic mass of O is 15.9994 , and we have
100.00 − 36.84 = 63.16 g O :
63.16 g N
15.9994 g N/mol N = 3.948 mol N
Now the ratio 3.958 /2.630 is very close to 1.5 = 3 2 . So we conclude that the gas has three moles O to two moles N making the empirical formula N 2 O 3 .
Explanation: