<u>Answer:</u> Aluminium is getting oxidized in the given chemical reaction.
<u>Explanation:</u>
Oxidation reaction is defined as the chemical reaction in which an atom looses its electrons. The oxidation number of the atom gets increased during this reaction.

Reduction reaction is defined as the chemical reaction in which an atom gains electrons. The oxidation number of the atom gets reduced during this reaction.

For the given chemical reaction:

The half cell reactions for the above reaction follows:
<u>Oxidation half reaction:</u> 
<u>Reduction half reaction:</u> 
As, aluminium is loosing 3 electrons to form aluminium cation. Thus, it is getting oxidized. Iron is gaining 2 electrons to form iron anion. Thus, it is getting reduced.
Hence, the oxidized species of the given reaction is aluminium.
Answer:
108 j
Explanation:
.24 j/g-C * 15 g * (55-25) =
The answer is: [D]: a reactant.
________________________
Answer:
M = 20.5 g/mol
Explanation:
Given data:
Volume of gas = 1.20 L
Mass of gas = 1.10 g
Temperature and pressure = standard
Solution:
First of all we will calculate the density.
Formula:
d = mass/ volume
d = 1.10 g/ 1.20 L
d = 0.92 g/L
Now we will calculate the molar mass.
d = PM/RT
0.92 g/L = 1 atm × M / 0.0821 atm.L/mol.K ×273.15 K
M = 0.92 g/L × 0.0821 atm.L/mol.K ×273.15 K / 1 atm
M = 20.5 g/mol