Answer:
d. 4 Al(s) + 3 O₂(g) → 2 Al₂O₃(s)
Explanation:
Aluminum metal reacts with oxygen gas in a combination reaction that forms a product that coats the metal preventing it from further oxidation: aluminum oxide. Aluminum is a cation with charge 3+ (Al³⁻) and oxide is an anion with charge 2- (O²⁻). Thus, the neutral compound aluminum oxide has the chemical formula Al₂O₃. The unbalanced chemical equation is:
Al(s) + O₂(g) → Al₂O₃(s)
We can balance using the trial and error method. First, we will balance O atoms by multiplying Al₂O₃ by 2 and O₂ by 3.
Al(s) + 3 O₂(g) → 2 Al₂O₃(s)
Finally, we get the balanced equation by multiplying Al by 4.
4 Al(s) + 3 O₂(g) → 2 Al₂O₃(s)
Explanation:
carbon dioxide has a percent composition of 72.7% oxygen, i.e. for every 100 g of carbon dioxide you get 72.7 g of oxygen.
Answer: The pressure in torr is 461 torr
Explanation:
To calculate the relation of density and molar mass of a compound, we use the ideal gas equation:
PV=nRT
P = pressure
V = Volume
n = number of moles
R = gas constant = 0.0821 Latm/Kmol
T = temperature =
Number of moles (n) can be written as:
where, m = given mass
M = molar mass = 44 g/mol
where,
where d = density = 2.54 g/L
The relation becomes:
PM=dRT
(760torr=1atm)
Thus the pressure in torr is 461 torr
