Darkblade48

I believe chlorine atoms were green and sulfur were yellow.

Well, I can safely say that 14) means that you're going to ignore chirality, i.e. R and S enantiomers.

I have found about half of these and I would greatly appreciate help...thanks for your help in advance.

5. Compound formed by an alkali and a halogen.

If you mean alkali metal, then look no further than your kitchen for a compound that is formed between an alkali metal and a halogen.

12. Solution of an isomer of CH3-CH2-CH2OH.

Try drawing the molecule out, and placing the OH in various locations

25. Ionic sunstance whose lattice energy is greater than its hydration energy.

Look for compounds that, when added to water, cool down the solution

To ecoli: IMO, it sure seems like homework...

t used in some boat yards also as Cathodic protection, but you`de need a car to move one!

I thought these were more commonly made of zinc?

??? Zinc has a higher atomic number (30) than calcium (20)

Mainly due to hyperconjugation (i.e. the interaction of electrons from the carbon next to the carbocation will tend to have a stabilizing effect on the cation).

In addition, benzylic and allylic carbocations are even more stable.

The Sn1 nucleophilic substitution cannot be applied to a primary haloalkane because of the instability of the carbocation that would be formed (i.e. a tertiary carbocation is much more stable than a primary carbocation).

Similarly for electrophilic substitution, this occurs on aromatic rings and not alkenes because of the stability of the resulting arenium ion (i.e. due to resonance). On an alkene, no such resonance can occur, and thus it is less stable.

According to an MSDS I found, about 825 C.

You shouldn't omit the word "sodium" from "sodium chloride". After all, NaCl is sodium chloride, like you said.

Your equation is also incorrect; another product of the reaction is water.

Using ammonium nitrate to show off endothermic properties is always fun (i.e. put a drop of water on a piece of wood, and then mix ammonium nitrate into a flask, put on top of the drop of water. It'll freeze, and you can freely lift up the block of wood).

Bismuth metal can be heated up and if cooled down slowly, you can form beautiful crystals (I'd do the heating in a crucible).

Zinc dust is a good reductor for many reactions.

You can make methylsalicylate if you have the salicylic acid. It's a little early in the morning for me, so I can't quite remember how to convert the ASA to SA, but it's definitely possible; perhaps if I remember I'll edit this post

These sound suspiciously like homework problems to me...

What you said is true; volume does not play a role because of the number of particles (i.e. a 10 ml solution of 1 M HCl would react with metal slower than a 10 ml solution of 10 M HCl would).

However, in terms of surface area, volume might matter. For example, imagine a small tube filled with a 1 M solution of HCl making contact with a piece of metal (small surface area) vs. a large diameter tube filled with the same volume of 1 M HCl making contact with another piece of metal.

Obviously, the larger diameter tube will have more surface area available for the metal/acid interaction to occur (i.e. the volume of acid is spread out over more surface area)

Sounds fine, though when you say "quantity" you must clarify that you are referring to moles and not to volume.

I believe it's because of the nature of AC power (i.e. the current alternates, 60 Hz a second), causing the cathode/anode to switch just as rapidly. This means no real electrolysis occurs.

Please show that you have put at least some effort into trying to do questions like these...

Hint: Try looking at colligative properties and the osmotic pressure formula, which is:

(pi)(V) = nRT

At the point of inflection of the titration curve, a small change in the concentration of acidic or basic ions will result in a large change.

so if you are looking for wether or not hcl is reactive with a metal, a change in color of the metal would not be something to look for?

I would not look for a colour change, no. I can think of several metals that will react with hydrochloric acid that do not elicit a colour change.

You would simply need to look up the phase diagrams for your various gases (assuming they are pure) in order to find the pressure and/or temperature required to liquify them.

It is unlikely you would be able to store a gas as a liquid in a glass container for any period of time, however. The pressure required to keep gases liquified will exceed the ability of the glassware to withstand implosion.

Metals don't change colour upon reacting with hydrochloric acid; unless, perhaps, you're thinking of transition metals and their salts?

Please show that you've made an attempt at this (homework) problem.

my dad has this thick metallicy stuff i, you can bend it east and he said it would protect radiant heat easily, it starts with a M. My dads a senior captain firefighter so he knows a lot about hazmat and science things.

You're probably referring to Mylar in this case.

I've always thought of experimental error as a more "general" term to errors. For example, if you forgot (I certainly hope you didn't though!) to add a specific reagent, or perhaps contaminated one of your reagents accidently, this could be considered experimental error. Surely, you can't call this percentage of error, as it'd be impossible to arrive at a calculable numerical answer.

Take your mass of KIO3 and dissolve in 100 ml water to obtain your 0.01M solution.

Hint: You can use an ICE (initial, change, equilibrium) table in order to solve this question. You have your initial concentrations, you know the change will be some "x", and thus, you have your change, and can equate the values to your K(eq) and solve for the unknown "x".