Rust off!

2025-04-22T23:24:22+00:00

Yo, listen up!

dat Rust crew's been pushin' hard to get their language into the Linux kernel, but let's take a step back and examine their priorities, 'kay?
They're all about Rust, Rust, Rust - but what about the stability and maintainability of the kernel?
I'm talkin' about the millions of users who rely on Linux, not just some niche group of devs who wanna play with the latest shiny thing.
Take marcan, the Asahi Linux lead, for example.
He's been ragin' about the kernel community bein' resistant to change, but when you look at his own actions, it's clear his priority is gettin' Rust into the kernel, no matter what.
He's talkin' about burnout, but it seems like he's more burnt out on the kernel community's cautious approach than on actually gettin' the job done.
He be pushin new complexities and work on other people who are not interested in his fetish.
We're just trying to ensure that any changes to the kernel are thoroughly tested and validated.
I mean, come on, they're the ones who are tryin' to introduce a whole new language into the kernel - shouldn't they be the ones demonstratin' a willingness to work with the community and address our concerns?
It's like they're more interested in provin' a point - that Rust can be used in the kernel - than in actually contributin' to the Linux ecosystem in a meaningful way.
And that's just not cool, bro. We're talkin' about a critical piece of infrastructure here, not some playground for language enthusiasts.
So, yeah, I'm suspicious of their priorities. It seems like they're more about promotin' Rust than about doin' what's best for Linux.
And if that's the case, then we need to take a step back and re-evaluate their contributions.
The kernel community's not against innovation, but we're not gonna sacrifice stability and maintainability on the altar of some new language or framework, either.

Reply to thread

2025-04-23T04:30:06+00:00

Hello, Animal Crossing cap'n.

Reply to thread

2025-05-26T21:02:53+00:00

There are several easy ways to remove rust using common household items:

1. Vinegar:Submerge the rusty item in white vinegar for several hours or overnight. For larger items, soak a cloth in vinegar and wrap it around the rusted area. Scrub off the loosened rust with a brush or steel wool. Rinse and dry the item thoroughly.

2. Baking Soda: Make a paste of baking soda and water. Apply the paste to the rusted area and let it sit for a few hours. Scrub the rust away with a brush or steel wool. Rinse and dry the item.

3. Lemon or Lime Juice with Salt: Sprinkle salt generously over the rusted area. Squeeze lemon or lime juice over the salt. Let the mixture sit for a few hours. Scrub the rust away with the rind of the fruit or a brush. Rinse and dry the item.

4. Potato and Dish Soap: Cut a potato in half and cover the cut side with dish soap. Use the potato to scrub the rusted area. The oxalic acid in the potato helps to dissolve rust. Rinse and dry the item.

5. Cola: Soak the rusty item in cola for several hours or overnight. The phosphoric acid in cola helps to break down rust. Scrub off any remaining rust and rinse and dry the item.

Important Considerations:

Severity of Rust: These methods work best for light to moderate rust. For heavy rust, you may need to repeat the process or use a commercial rust remover.

Material: Some of these methods may not be suitable for all materials. For example, vinegar can damage painted surfaces.

Safety: Wear gloves when using any rust removal method, especially commercial products. Ensure good ventilation if using chemical rust removers.

Elbow Grease: Most of these methods will require some scrubbing to remove the rust effectively.

Choose the method that best suits the rusted item and the severity of the rust. Remember to always rinse and dry the item thoroughly after removing rust to prevent it from returning.

Reply to thread

2025-06-09T20:28:58+00:00

Rust, commonly known as iron oxide, is a reddish-brown flaky substance that forms on iron and its alloys (like steel) when they are exposed to oxygen and water. It's a prime example of corrosion, an electrochemical process where metals deteriorate through redox reactions.

The formation of rust is a complex process involving several steps, but it can be summarized as the oxidation of iron in the presence of water and oxygen.

Key Requirements for Rust Formation:

Iron (Fe): The metal itself.
Oxygen (O₂): From the air or dissolved in water.
Water (H₂O): Essential for the electrochemical reactions. The presence of electrolytes (like salts) and acidic conditions in the water can significantly accelerate the rusting process.

Mechanism and Chemical Reactions:

Rusting is an electrochemical process, meaning it involves both oxidation and reduction reactions occurring simultaneously.

Oxidation of Iron (Anode):
At certain points on the iron surface (anodic areas), iron atoms lose electrons and are oxidized to iron(II) ions (Fe2+).
Fe(s)→Fe2+(aq)+2e−
These electrons then travel through the iron metal to other areas (cathodic areas).

Reduction of Oxygen (Cathode):
At the cathodic areas, oxygen dissolved in the water gains the electrons released by the iron. This reduction of oxygen typically occurs in the presence of water to form hydroxide ions (OH−).
O2(g)+2H2O(l)+4e−→4OH−(aq)
If the water contains acidic substances (like dissolved carbon dioxide forming carbonic acid), hydrogen ions can also be involved in the reduction:
4H+(aq)+O2(g)+4e−→2H2O(l)

Formation of Iron(II) Hydroxide:
The Fe2+ ions produced at the anode react with the OH− ions produced at the cathode to form iron(II) hydroxide.
Fe2+(aq)+2OH−(aq)→Fe(OH)2(s)

Oxidation of Iron(II) Hydroxide:
Iron(II) hydroxide is then further oxidized by oxygen to form iron(III) hydroxide.
4Fe(OH)2(s)+O2(g)+2H2O(l)→4Fe(OH)3(s)

Dehydration to Form Hydrated Iron(III) Oxide (Rust):
Iron(III) hydroxide is unstable and dehydrates to form hydrated iron(III) oxide, which is commonly known as rust. The exact composition of rust varies, but it's generally represented as Fe2O3⋅nH2O, where 'n' represents a variable number of water molecules.
2Fe(OH)3(s)→Fe2O3⋅nH2O(s)+(3−n)H2O(l)

Overall Simplified Reaction:

While the process is complex, a simplified overall chemical equation for rust formation is often given as:

4Fe(s)+3O2(g)+6H2O(l)→4Fe(OH)3(s)

Which then dehydrates to form:

4Fe(s)+3O2(g)+xH2O(l)→2Fe2O3⋅xH2O(s)

Factors that Accelerate Rusting:

Presence of Electrolytes: Salts (like in saltwater) increase the electrical conductivity of the water, facilitating the movement of ions and speeding up the electrochemical reactions.

Acidity (Low pH): Acidic conditions promote the oxidation of iron.
Temperature: Higher temperatures generally increase the rate of chemical reactions.
Presence of Impurities: Impurities in the iron can create tiny electrochemical cells, accelerating rusting.

Unlike protective oxide layers that form on some metals (like aluminum, which forms a tightly adhering aluminum oxide layer that prevents further corrosion), the rust layer on iron is typically porous and flaky. This allows oxygen and water to continue to reach the underlying metal, leading to further corrosion and ultimately weakening the iron object.