Be sure to answer all parts. For the complete redox reactions given here, write the half-reactions and identify the oxidizing and reducing agents. Make sure your answer has the simplest coefficients. Part 1 out of 4 (a) 4Fe + 3O2 → 2Fe2O3 Select the oxidizing agent:

Answer : is the oxidizing agent and Fe is the reducing agent.

Explanation :

Reducing agent : It is defined as the agent which helps the other substance to reduce and itself gets oxidized. Thus, it will undergo oxidation reaction.

Oxidizing agent : It is defined as the agent which helps the other substance to oxidize and itself gets reduced. Thus, it will undergo reduction reaction.

The balanced redox reaction is :

The half oxidation-reduction reactions are:

Oxidation reaction :

Reduction reaction :

In order to balance the electrons, we multiply the oxidation reaction by 4 and reduction reaction by 3 then added both equation, we get the balanced redox reaction.

Oxidation reaction :

Reduction reaction :

In this reaction, is the reducing agent that loses an electron to another chemical species in a redox chemical reaction and itself gets oxidized and is the oxidizing agent that gain an electron to another chemical species in a redox chemical reaction and itself gets reduced.

Thus, is the oxidizing agent and Fe is the reducing agent.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.