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grin007 [14]
2 years ago
10

Using 21st-century technology, hydrogen fusion requires temperatures around 10^8 K. But, lower initial temperatures are used if

the hydrogen is compressed. In the late 24th century, the starship Leinad uses such methods to fuse hydrogen at 10^6 K.(e) Should the captain of the Leinad change the technology and produce ³He (mass = 3.01603 amu) instead of ⁴He?
Chemistry
1 answer:
Bezzdna [24]2 years ago
3 0

<u>No, the captain should continue using the current technology.</u>

<u></u>

<h3>How Nuclear Fusion Reactors Work?</h3>

­W­hen hydrogen atoms fuse, the nuclei must come together. However, the protons in each nucleus will tend to repel each other because they have the same charge (positive). If you've ever tried to place two magnets together and felt them push apart from each other, you've experienced this principle firsthand.

To achieve fusion­, you need to create special conditions to overcome this tendency. Here are the conditions that make fusion possible:

High temperature gives the hydrogen atoms enough energy to overcome the electrical repulsion between the protons.

  • Fusion requires temperatures of about 100 million Kelvin (approximately six times hotter than the sun's core).
  • At these temperatures, hydrogen is a plasma, not a gas. Plasma is a high-energy state of matter in which all the electrons are stripped from atoms and move freely about.
  • The sun achieves these temperatures by its large mass and the force of gravity compressing this mass in the core. We must use energy from microwaves, lasers and ion particles to achieve these temperatures.

High pressure squeezes the hydrogen atoms together. They must be within 1x10-15 meters of each other to fuse.

  • The sun uses its mass and the force of gravity to squeeze hydrogen atoms together in its core.
  • We must squeeze hydrogen atoms together by using intense magnetic fields, powerful lasers or ion beams.

Learn more about Fusion

brainly.com/question/9464925

#SPJ4

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Answer:

1.24 × 10³ kPa

Explanation:

Step 1: Given data

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Step 2: Calculate the final pressure of the gas in the can

If we assume that the gas in the can behaves as an ideal gas and that the temperature remains constant, we can calculate the final pressure of the gas using Boyle's law.

P₁ × V₁ = P₂ × V₂

P₂ = P₁ × V₁ / V₂

P₂ = 34.5 kPa × 473 mL / 13.16 mL = 1.24 × 10³ kPa

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