Explanation: 63.546 + (14.0067 + 15.9994*3)*2
Number of moles of Al produced = 11 moles
Number of moles of oxygen produced = ?
To solve this problem, we need to understand the problem.
The decomposition of an aluminium oxide must has produced oxygen and aluminium,
2Al₂O₃ → 4Al + 3O₂
now since the known is the oxygen gas; we can find the unknown aluminium:
3 mole of O₂ was produced with 4 mole of Al
x mole of O₂ will be produced with 11 moles of Al
x = = 8.25 moles
2NO2 ⇆ N2O4 + 57.2 kj
what happen when temperature of the above reaction is increased is
more product forms
The empirical formula is: Fe(CO)₅
According the global reaction:
Feₓ(CO)y + O₂ → Fe₂O₃ + CO₂
You should calculate Fe₂O₃ and CO₂ moles, thus:
0,799 Fe₂O₃ grams × = 5,00×10⁻³ Fe₂O₃ moles
2,200 CO₂ grams × = 5,00×10⁻²CO₂ moles
The ratio between Fe₂O₃ moles and CO₂ moles is 1:10. Thus ratio between x and y must be 1:5 because Fe₂O₃ has 2 irons but CO₂ has just one carbon.
Assuming the formula is Fe₁(CO)₅ the molecular weight is 195,9 g/mol. Thus:
1,959 Fe(CO)₅ grams × = 1,00×10⁻² Fe(CO)₅ moles
Thus, assuming 1,00×10⁻² moles as basis for calculation, the global reaction is:
1 Fe(CO)₅ + ¹³/₂O₂ → ¹/₂ Fe₂O₃ + 5 CO₂
With this balanced equation the moles produced have sense, thus, the empirical formula is: Fe(CO)₅
I hope it helps!
1. 1086.04 mmHg
3. 95.954 kPa
Pressure (P) is the force applied per unit area
Can be formulated :
P = pressure (SI=Pascal(Pa))
F= force applied (N)
The unit of pressure can be expressed in atm, mmHg, or Pascal