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3 years ago

2) Which element is used as fuel in nuclear reactors? How many years before we run out of it?

Chemistry

1 answer:

Firlakuza [10]3 years ago

5 0

Answer:Uranium

80 years

To make that nuclear reaction that makes that heat, those uranium pellets are the fuel. And just like any fuel, it gets used up eventually. Your 12-foot-long fuel rod full of those uranium pellet, lasts about six years in a reactor, until the fission process uses that uranium fuel up.

Transuranic wastes, sometimes called TRU, account for most of the radioactive hazard remaining in high-level waste after 1,000 years. Radioactive isotopes eventually decay, or disintegrate, to harmless materials. Some isotopes decay in hours or even minutes, but others decay very slowly.

Explanation:

Hope this helps

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If 56 grams of notrogen are used up by the reaction, how many grams of amonia will be produced? 1N2+3H2--> 2NH3

djverab [1.8K]

1 mole of N2 produces 2 moles of NH3
OR...
14 x 2 grams of N2 produces 2(14 +3) grams of NH3
1 gram of N2 produces 34/28 grams of NH3
therefore, 56 grams produce (34/28 )x 56 =68 grams of NH3

the answer thus would be 68 grams of NH3

5 0

3 years ago

Answer the question below based on the periodic table entry for bromine.

Shalnov [3]

<span>The number of neutrons bromine will have are equal to
= protons + neutrons
so,
80-35=45</span>

4 0

3 years ago

Read 2 more answers

You have 2.7 moles of carbon. How many atoms do you have?

Gelneren [198K]

Answer:

1.63 × 10²⁴ atoms.

Explanation:

To calculate the number of atoms (N) contained in 2.7moles of carbon, we multiply the number of moles (n) by Avogadro's number (6.02 × 10²³).

That is, N = n × nA

Where;

N = number of atoms

n = number of moles (mol)

nA = Avogadro's numbe

N = 2.7 × 6.02 × 10²³

N = 16.254 × 10²³

N = 1.63 × 10²⁴ atoms.

Hence, there are 1.63 × 10²⁴ atoms in 2.7moles of Carbon.

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3 years ago

The molar heat of fusion for water is 6.01 kJ/mol. How much energy must be added to a 75.0-g block of ice at 0°C to change it to

andreyandreev [35.5K]

Answer is: 25,06 kJ of energy must be added to a 75 g block of ice.
ΔHfusion(H₂O) = 6,01 kJ/mol.
T(H₂O) = 0°C.
m(H₂O) = 75 g.
n(H₂O) = m(H₂O) ÷ M(H₂O).
n(H₂O) = 75 g ÷ 18 g/mol.
n(H₂O) = 4,17 mol.
Q = ΔHfusion(H₂O) · n(H₂O)
Q = 6,01 kJ/mol · 4,17 mol
Q = 25,06 kJ.

7 0

3 years ago

Read 2 more answers

Find the mass in grams of 3.00 x 1023 molecules of F2

LUCKY_DIMON [66]

<h3>Answer:</h3>

18.9 g F₂

<h3>General Formulas and Concepts:</h3>

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

Brackets
Parenthesis
Exponents
Multiplication
Division
Addition
Subtraction

Left to Right

<u>Chemistry</u>

<u>Atomic Structure</u>

Reading a Periodic Table
Using Dimensional Analysis
Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.

<h3>Explanation:</h3>

<u>Step 1: Define</u>

3.00 × 10²³ molecules F₂

<u>Step 2: Identify Conversions</u>

Avogadro's Number

Molar Mass of F₂ (Diatomic) - 38.00 g/mol

<u>Step 3: Convert</u>

Set up: $\displaystyle 3.00 \cdot 10^{23} \ molecules \ F_2(\frac{1 \ mol \ F_2}{6.022 \cdot 10^{23} \ molecules \ F_2})(\frac{38.00 \ g \ F_2}{1 \ mol F_2})$
Multiply: $\displaystyle 18.9306 \ g \ F_2$

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 3 sig figs.</em>

18.9306 g F₂ ≈ 18.9 g F₂

8 0

3 years ago