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Hoochie [10]
3 years ago
11

The model below represents a nuclear reaction. Atom 1 is present before the reaction and Atom 2 and Atom 3 are produced after th

e reaction.
Atom 1 = Atom 2 + Atom 3 + energy

The model most likely represents a reaction which
Select one:
a. takes place when atoms combine
b. takes place when atoms become inactive
c. does not produce energy in the sun
d. does not produce energy in nuclear power plants
Chemistry
2 answers:
Jet001 [13]3 years ago
8 0

Answer: b: takes place when atoms become inactive

Explanation: the model described above is a nuclear fission reaction, a reasonably controlled reaction that releases energy and is employed in nuclear power plants. In these reactions one Atom is split into two lighter ones and there's a resultant release of energy in the process. The original Atom becomes depleted (inactive) as is the case with Uranium 235.

This reaction is opposed to fusion reactions that occur in nature e.g. the sun, and are basically uncontrollable — involving the combination of two atoms into one.

belka [17]3 years ago
7 0
The right answer for the question that is being asked and shown above is that: "d. does not produce energy in nuclear power plants." The model most likely represents a reaction which d. does not produce energy in nuclear power plants<span>
</span>
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Le Châtelier's principle tells us that chemical _____ will adjust in an attempt to remove a stressor.
lawyer [7]
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8 0
3 years ago
how much hydrogen gas is necessary to exert a pressure of 1.4 ATM at 430k if occupying a volume of 15.1 l
lora16 [44]

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5

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7 0
3 years ago
For the following reaction, 22.9 grams of nitrogen monoxide are allowed to react with 5.80 grams of hydrogen gas. nitrogen monox
ololo11 [35]

Answer:

1) Maximun ammount of nitrogen gas: m_{N2}=10.682 g N_2

2) Limiting reagent: NO

3) Ammount of excess reagent: m_{N2}=4.274 g

Explanation:

<u>The reaction </u>

2 NO (g) + 2 H_2 (g) \longrightarrow N_2 (g) + 2 H_2O (g)

Moles of nitrogen monoxide

Molecular weight: M_{NO}=30 g/mol

n_{NO}=\frac{m_{NO}}{M_{NO}}

n_{NO}=\frac{22.9 g}{30 g/mol}=0.763 mol

Moles of hydrogen

Molecular weight: M_{H2}=2 g/mol

n_{H2}=\frac{m_{H2}}{M_{H2}}

n_{H2}=\frac{.5.8 g}{2 g/mol}=2.9 mol

Mol rate of H2 and NO is 1:1 => hydrogen gas is in excess

1) <u>Maximun ammount of nitrogen gas</u> => when all NO reacted

m_{N2}=0.763 mol NO* \frac{1 mol N_2}{2 mol NO}*\frac{28 g N_2}{mol N_2}

m_{N2}=10.682 g N_2

2) <u>Limiting reagent</u>: NO

3) <u>Ammount of excess reagent</u>:

m_{N2}=(2.9 mol - 0.763 mol NO* \frac{1 mol H_2}{1 mol NO})*\frac{2 g H_2}{mol H_2}

m_{N2}=4.274 g

8 0
3 years ago
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