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slega [8]
1 year ago
8

Describe the nature and purpose of these components of a nuclear reactor:(b) moderator;

Chemistry
1 answer:
sertanlavr [38]1 year ago
8 0

The moderator of a nuclear reactor is a substance that slows neutrons down. In traditional nuclear reactors, the moderator is the same thing as the coolant: it’s water! When fast neutrons strike the hydrogen atoms in H2O, they slow down a lot (like a billiard ball striking another). There are other good moderators like graphite, beryllium, and more.

<h3>What is moderator ?</h3>

Other neutrons are released at extremely high speeds when an incoming neutron splits an atom's nucleus. A sustained chain reaction is achievable if at least one (on average) of these neutrons can be made to split another fuel atom. In fact, if a neutron is traveling slowly, fuel atoms (like uranium) are more likely to absorb it (see Figure 1). In order to make a chain reaction easier to achieve, moderators are used in many reactor designs.

Neutrons can be slowed down more effectively in some materials than others. Because of the rules of conservation of energy and momentum, a neutron (mass 1) colliding with a heavy nucleus like a fuel atom cannot significantly slow down (mass 235).

To learn more about moderator  from the given link:

brainly.com/question/27936671

#SPJ4

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A solution of sugar contains 35 gramsof sucrose, C12H22O11in 100 mL of water. What is the percent composition of the solution?
KATRIN_1 [288]

Answer:

Percent composition of the solution is 26 % of sucrose and 74 % of water

Explanation:

Percent composition is the mass of solute, either of solvent in 100 g of solution.

Mass of solution = Mass of solvent + Mass of solute

Mass of solute = 35 g

Mass of solvent = 100 g

As we know, water density = 1g/mL

So 1g/mL . 100 mL = 100 g

35 g + 100 g = 135 g → Mass of solution

(Mass of solute / Mass of solution) . 100 =

(35 g / 135 g) . 100 = 26 %

(Mass of solvent / Mass of solution) . 100 =

(100 g / 135 g) . 100 = 74 %

8 0
2 years ago
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Answer:

a and d

Explanation:

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6 0
2 years ago
A 2.00-mol sample of hydrogen gas is heated at constant pressure from 294 K to 414 K. (a) Calculate the energy transferred to th
Furkat [3]

Answer:

a) The energy transferred is 6.91 kJ

b) The internal energy is 4.90 kJ

c) The work done on the gas is - 2.01 kJ

Explanation:

Step 1: Data given

Number of moles of hydrogen gas = 2.00 moles

Pressure = constant

Temperature is heated from 294 K to 414 K

Molar heat capacity of hydrogen gas = 28.8 J/mol*K

Step 2: Calculate the energy transferred to the gas by heat.

Q = n* Cp * ΔT

⇒with Q =the energy transferred

⇒with n = the number of moles = 2.00 moles

⇒with Cp = the Molar heat capacity of hydrogen gas = 28.8 J/mol*K

⇒ with ΔT = Temperature 2 - Temperature 1 = 414 - 294 = 120K

Q = 2.00 * 28.8 * 120

Q = 6912 J = 6.91 kJ

Step 3: Calculate the increase in its internal energy.

ΔEint = n*Cv*ΔT

⇒with ΔEint = the increase in its internal energy.

⇒with n = the number of moles = 2.00 moles

⇒with Cv = The constant volume = 20.4 J/mol*K

⇒with  ΔT = Temperature 2 - Temperature 1 = 414 - 294 = 120K

ΔEint = 2.00 * 20.4 * 120

ΔEint =4896 J = 4.90 kJ

Step 4: Calculate the work done on the gas.

Work done on the gas = -Q + ΔEint

W = -6.91 kJ + 4.90 kJ

W = -2.01 kJ

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3 years ago
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