Answer:
B) PO2
Explanation:
first solve empirical formula
50%of P and 50%of O
- divide each by molecular mass
P. O
50/32. 50/16
1.5. 3.0
- divide both by the smallest
1.5/1.5. 3.0/1.5
1. :. 2
Empirical formula=PO2
Molecular formula=PO2
(PO2)n= 64
(32+(16×2)=64
(32+32)n=64
64n=64
n= 1
Answer:
0.0059mol
Explanation:
From the ideal gas equation
PV=nRT
P=Pressure
V=Volume
R=Ideal gas constant
T=Temperature
n=number of mole
P=745mmHg
760mmHg=1atm
745mmHg=0.98atm
volume of water displaced=volume of hydrogen produced=145ml=0.145L
R=0.082Latm/mol/K
T=22°C=273+22=293K
no of mole=PV/RT
=0.98×0.145/0.082×293
=0.1421/24.026
=0.0059mol
1
Answer:
D. 2NH₃(g) ⟶ N₂(g) + 3H₂(g)
Explanation:
A chemical equation must show the correct formulas for reactants and products.
A and B are wrong, because they have NH₃ as a product.
C is wrong. H₃ does not exist.
A is correct. The equation for the decomposition of ammonia is
2NH₃(g) ⟶ N₂(g) + 3H₂(g)
A) occurs when water is evaporated.