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Georgia [21]
4 years ago
5

Which of the statements regarding the nitrogen cycle is true? choose 1 answer: choose 1 answer: a animals obtain nitrogen throug

h the process of cellular respiration. b atmospheric nitrogen is absorbed through the leaves of plants. c nitrogen fixation is the process atmospheric nitrogen is converted into biologically usable forms. d denitrification occurs when a nitrogen containing compound is produced from nitrogen in the soil?
Chemistry
2 answers:
Lera25 [3.4K]4 years ago
7 0
The nitrogen cycle requires different types of bacteria.
Leona [35]3 years ago
4 0

Answer: Option C

Explanation:

The nitrogen cycle can be defined as the process by which the nitrogen is being recycled. The nitrogen is transferred from the atmosphere to the plants and then from plants to animals, human beings.

Then from animals and human beings it is again transferred into the soil and then atmosphere.

The nitrogen that is found in the sol is not in the usable form by the plants, nitrogen fixing bacteria converts it into usable form.

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Consider the following unbalanced redox reactions. In each case, separate the whole reactions into half-reactions, balance the h
Marina86 [1]

Answer & Explanation:

(a)

Fe^{2+} +NO_{3}^{-}  => Fe{(OH)}_3 + N_2

reducing agent = Fe²⁺

Oxidizing agent = NO₃⁻

oxidation

Fe²⁺  ⇒ Fe(OH)₃

reduction

NO₃⁻  ⇒ N₂

Oxidation Half Reaction

(<em>redox reactions are balanced by adding appropriate H⁺ and H₂O atoms)</em>

Fe²⁺ ⇒ Fe(OH)₃

Balance O atoms

Fe²⁺ + 3H₂O ⇒ Fe(OH)₃

Balance H atoms

Fe² + 3H₂0 ⇒ Fe(OH)₃ + 3H⁺

balance Charge

Fe² + 3H₂0 ⇒ Fe(OH)₃ + 3H⁺ + e⁻..............(1)

reduction Half Reaction

NO₃⁻ ⇒ N₂

Balance N atoms

2NO₃⁻ ⇒N₂

Balance O atoms by adding appropriate H₂O

2NO₃⁻ ⇒ N₂ + 6H₂O

Balance H atoms

2NO₃⁻ + 12H⁺ ⇒ N₂ + 6H₂O

Balance Charge

2NO₃⁻ + 12H⁺ + 10e⁻⇒ N₂ + 6H₂O.................(2)

Combine Equation (1) and (2)

(1) × 10: 10Fe² + 30H₂0 ⇒ 10Fe(OH)₃ + 30H⁺ + 10e⁻

(2) × 1:   2NO₃⁻ + 12H⁺ + 10e⁻⇒ N₂ + 6H₂O

(1) + (2): 10Fe² + <u><em>30H₂0</em></u> + 2NO₃⁻ + <u><em>12H⁺</em></u> + <u><em>10e⁻</em></u> ⇒10Fe(OH)₃ + <u><em>30H⁺</em></u><u><em> </em></u>+ <em><u>10e⁻</u></em> +              

            N₂ + <u><em>6H₂O</em></u>

            10Fe² + 24H₂0 + 2NO₃⁻  ⇒ 10Fe(OH)₃ + 18H⁺ + N₂

this is the balanced reaction

REDUCTION POTENTIAL

10Fe²⁺(aq) + 10e⁻ ⇒ 10Fe(OH)₃(aq)             E°ox = 10(-0.44) = -4.4V

2NO₃⁻(aq) -  2e⁻ ⇌ N₂(g) + 18H⁺       E°red = 2(+0.80) = +1.6

10Fe² + 24H₂0 + 2NO₃⁻  ⇒ 10Fe(OH)₃ + 18H⁺ + N₂    E°cell = -2.8V

E°cell = E°red + E°ox

4 0
4 years ago
Convert 16 inches to feet
MrRa [10]

There is 12 inches in 1 foot.

Divide 16 with 12 to get feet

16/12 = ~1.33 (rounded)

1.33 is your answer

hope this helps

5 0
4 years ago
Read 2 more answers
Given the following balanced equation, determine the rate of reaction with respect to [O2]. If the rate of formation of O2 is 7.
murzikaleks [220]

Answer: The rate of the loss of O_3 is 0.52M/s

Explanation:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

The rate in terms of reactants is given as negative as the concentration of reactants is decreasing with time whereas the rate in terms of products is given as positive as the concentration of products is increasing with time.

2O_3(g)\rightleftharpoons 3O_2(g)

Rate of disappearance of O_3 =-\frac{1d[O_3]}{2dt}

Rate of formation of O_2 =+\frac{1d[O_2]}{3dt}

-\frac{1d[O_3]}{2dt}=+\frac{1d[O_2]}{3dt}

Rate of formation of O_2 = 7.78\times 10^{-1}M/s

Thus Rate of disappearance of O_3 =\frac{2d[O_2]}{3dt}=\frac{2}{3}\times 7.78\times 10^{-1}M/s=0.52M/s

8 0
4 years ago
If a sample of 4 moles of gas has a pressure of 567.42 kPa and a volume of 12.0 L, what is it's temperature?
Lady_Fox [76]
Your answer is b, hope this helps ;)
7 0
3 years ago
Read 2 more answers
The specific heat of aluminum is 0.902 J/g C. If a one gram sample of aluminum absorbs 50 Joules of energy, how much with its te
PtichkaEL [24]
Answer:
55.4324℃
Explanation:
Q=cm△t
50J = 0.902J/(g·℃) x 1g x △t
△t =55.4324℃
7 0
3 years ago
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