What is the reducing agent in the reaction below? CrO3 + 2Al Cr + Al2O3

Chemistry

2 answers:

saveliy_v [14]3 years ago

8 0

<u>Answer: </u>The reducing agent of the given chemical reaction is

<u>Explanation:</u>

Reducing agent is defined as the agent which reduces the other substance and itself gets oxidized. It undergoes oxidation reaction. Oxidation reaction is defined as the reaction in which a substance looses its electron. The oxidation state of the substance gets increased.

Oxidizing agent is defined as the agent which oxidizes the other substance and itself gets reduced. It undergoes reduction reaction. Reduction reaction is defined as the reaction in which a substance gains electron. The oxidation state of the substance gets reduced.

For the given chemical reaction:

$CrO_3+2Al\rightarrow Cr+Al_2O_3$

On reactant side:

Oxidation state of chromium = +5

Oxidation state of aluminium = 0

Oxidation state of oxygen = -2

On product side:

Oxidation state of chromium = 0

Oxidation state of aluminium = +3

Oxidation state of oxygen = -2

As, oxidation state of aluminium is getting increased from 0 to +3. Thus, it is getting oxidized and considered as reducing agent. The oxidation state of chromium is getting reduced from +5 to 0. Thus, it is getting reduced and is considered as oxidizing agent.

Hence, the correct answer is aluminium.

DerKrebs [107]3 years ago

5 0

The answer is B. Al. Al is oxidized so it is the reducing agent

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How many miles of a gas at 100 c does it take to fill a 1.00 l flask to a pressure of 152kPa

Hatshy [7]

The complete question is as follows: How many moles of a gas at 100 c does it take to fill a 1.00 l flask to a pressure of 152kPa

Answer: There are 0.0489 moles of a gas at $100^{o}C$ is required to fill a 1.00 l flask to a pressure of 152kPa.

Explanation:

Given: Volume = 1.00 L,

Pressure = 152 kPa (1 kPa = 1000 Pa) = 152000 Pa

Convert Pa into atm as follows.

$1 Pa = 9.86 \times 10^{-6} atm\\152000 Pa = 152000 \times \frac{9.86 \times 10^{-6}atm}{1 Pa}\\= 1.5 atm$

Temperature = $100^{o}C = (100 + 273) K = 373 K$

Using the ideal gas formula as follows.

PV = nRT

where,

P = pressure

V = volume

n = no. of moles

R = gas constant = 0.0821 L atm/mol K

T = temperature

Substitute the values into above formula as follows.

$PV = nRT\\1.5 atm \times 1.0 L = n \times 0.0821 L atm/mol K \times 373 K\\n = \frac{1.5 atm \times 1.0 L}{0.0821 L atm/mol K \times 373 K}\\n = 0.0489 mol$