Answer:
1.5217391304348 gram/cubic centimeter is the density
3.5 gram/2.3 cubic centimeter
273 Kelvin, 0 degrees Celsius, 32 degrees Fahrenheit
Answer:
Explanation:
2Al(s) + 3 2 O2(g) → Al2O3(s) And given the stoichiometry ...and EXCESS dioxygen gas...we would get 6.25⋅ mol of alumina. the which represents a mass... ...6.25 ⋅ mol ×101.96 ⋅ g ⋅ mol−1 molar mass of alumina ≡ 637.25 ⋅ g.
Answer:
5.00 and 2.50 moles of aqueous sodium and sulfide ions are formed.
Explanation:
The dissociation reaction of sodium sulfide is as follows.
![Na_{2}S(aq)\rightarrow 2Na^{+}(aq)+S^{2-}(aq)](https://tex.z-dn.net/?f=Na_%7B2%7DS%28aq%29%5Crightarrow%202Na%5E%7B%2B%7D%28aq%29%2BS%5E%7B2-%7D%28aq%29)
From the reaction one mole of sodium sulfide produce 2 moles sodium ions.
Let's calculate the moles of
ions.
![Moles\,of\,Na^{+}=2.50molNa_{2}S\times \frac{2mol\,Na^{+}}{1mol\,Na_{2}S}=5.00mol\,Na^{+}](https://tex.z-dn.net/?f=Moles%5C%2Cof%5C%2CNa%5E%7B%2B%7D%3D2.50molNa_%7B2%7DS%5Ctimes%20%5Cfrac%7B2mol%5C%2CNa%5E%7B%2B%7D%7D%7B1mol%5C%2CNa_%7B2%7DS%7D%3D5.00mol%5C%2CNa%5E%7B%2B%7D)
From the reaction one mole of sodium sulfide produce one mole of sulfide ions.
Let's calculate the moles of
ions.
![Moles\,of\,S^{2-}=2.50molNa_{2}S\times \frac{1mol\,S^{2-}}{1mol\,Na_{2}S}=2.50mol\,S^{2-}](https://tex.z-dn.net/?f=Moles%5C%2Cof%5C%2CS%5E%7B2-%7D%3D2.50molNa_%7B2%7DS%5Ctimes%20%5Cfrac%7B1mol%5C%2CS%5E%7B2-%7D%7D%7B1mol%5C%2CNa_%7B2%7DS%7D%3D2.50mol%5C%2CS%5E%7B2-%7D)