In the given question,
HgxOy (2.50 g) = xHg (2.405 g) + yO
Here, mass of oxygen = 2.50 - 2.405
= 0.095 g
The moles of O₂ = 0.095 / 16 = 0.00594 moles
Moles of Hg = 2.405 / 200.60 = 0.01198 moles
Thus, the ratio of Hg : O is,
0.00594 : 0.01198 or 1 : 2
As the ratio is 1 : 2, thus, the empirical formula is Hg₂O
Answer:
The necessary equations necessary are explained in each step in the solution.
Explanation:
For conversion of methanol gas at 65°C to -112°C
the equations would be as follows,
step 1 : gas at 65°C to liquid at 65°C
q = n(-37 kJ/mol)
step 2 : liquid at 65°C to liquid at -94°C
q = n(81.1 J/mol°C), where dT is negative
step 3 : liquid at -94°C to solid at -94°C
q = n(-3.18 kJ/mol)
step 4 : solid at -94°C to solid at -112°C
q = n(48.7 J/mol°C), where dT is negative
The balanced equation is:
C3H8 + 5O2 > 3CO2 + 4H2O.
It takes 5 molecules of O2