Has anyone here done an experiment where you add MgO to HCl in a calorimeter?
955628
For the reaction:\n\nMgO + 2 HCl  -->  MgCl2 + H2O\n\nThe temperature should go up, not down.  Only the initial and final temperature are needed.\n\nTypical values for students are between 110 an 150 kJ/mol MgO.  This is typical, not the best that can be done.
743618
Commercially a safety fuse of gunpowder is used to ignite the mixture.\n\nUsing magnesium is an unreliable and perhaps a dangerous way of igniting thermite. This is because the igniting would usually be done through a small hole. This does not give the Mg enough oxygen to burn. It is dangerous because the heat generated by burning one end of the magnesium may propagate to the unburnt end due to the high heat conductivitity. This may cause premature ignition of the thermite.\n\nWell, in using Mg you may increase the contact area to air around the contact point around the Mg and the thermite.\n\nAlternatively, you could use a conventional sparkler to ignite the mixture.
138848
Here is one example ,\n\nAgNO3(aq) + NaCl(aq)-> AgCl(s)white precipitate + NaNO3(aq)
106494
First, distill off the alcohol. With ethanol, the best you can get is 95% purity, the remaining 5% is water. There are cheap zeolites and hygroscopic salts such as CaCl2 or NaOH available which can further reduce the amount of water. If you are still not happy, you can get absolute alcohols by using magnesium. And magnesium ribbons or turnings are relatively cheap, too. Place (50-100 g) magnesium in a flask, put some amount of alcohol just to cover the magnesium. Leave for a few hours until you see white magnesium alkoxide being formed on the surface of the metal. Caution: exothermic reaction. Use the tallest distillation column you can find. Do not stir the mixture. Just leave it there. When you have now a lot of magnesium alkoxide you can add more alcohol (up to 2 liters). The alkoxide will destroy any water in the alcohol and you now can distill off your absolute alcohols. For methanol and ethanol, formation of the alkoxide takes only a few hours. For other alcohols, you might need to activate the magnesium by adding some solid iodine and heating to activate the magnesium. Don't distill to dryness. The remaining alkoxide reacts violently with water. Use alcohol-water mixture when disposing them. Sounds fun, doesn't it? =)
608403
NaOH (aq) + HCl (aq) --> NaCl (aq) + H2O (l)
883152
MgO and BaO will react with water to form the hydroxides Mg(OH)2 and Ba(OH)2, those will be neutralized by hydrochloric acid to give the chlorides MgCl2 and BaCl2 and water.  I think you may have gotten C2O wrong, that is not a real chemical compound.  If you meant CaO it will behave in the same way as MgO and BaO.
1184412
Yes, in fact that has been done throught the concept of "Thermo-coupling" but again this method is economically infeasible, because the current generated in the process is in nano amperes.\nor in very small qty.
450756
That's a perfectly reasonable experiment.  It addresses issues of solubility and phase equilibria.  As long as the project is done in a logical manner (i.e. following the scientific method), it should be a good project.
299527
This may be what you are looking for:\n\nhttp://www.diva-portal.org/ntnu/abstract.xsql?dbid=104\n\nIt was the fifth entry in a search for "electrochemical MgO" in yahoo.
972791
HCl + NH4OH → H2O + NH4Cl.\nThere would be heat given off, so you could verify that a reaction took place.\n\n2HCl + Ca(OH)2 → 2H2O + CaCl2\n\nedit: The steps for balanacing the reaction:\n1)We know the salt produced is CaCl2, so an acid with Cl is HCl and a base with Ca is Ca(OH)2. \n2) write the skeleton reaction:\nHCl + Ca(OH)2 → H2O + CaCl2\n3) there are 2 Cl's on the right side, but only 1 on the left. To balance this, place a 2 in front of HCl\n2HCl + Ca(OH)2 → H2O + CaCl2\n4) Now there are 4 H on the left and only 2 on the right, so, place a 2 in front of H2O.\n2HCl + Ca(OH)2 → 2H2O + CaCl2\n5) check with the other elements, each side has one Ca, and 2 O. It all works out ☺
429367
It doesn't form into anything. You said it yourself, it's soluble. The hydroxide part of the milk of magnesia (magnesium hydroxide) and the hydrogen of the sulfuric acid combine to form water, but then you're left with Mg+2 and HSO4- ions. It's just a clear liquid.
882396
ummmm, maybe increase by a factor of 5 or so. Its an exothermic reaction to begin with and you're not limited by the amount of water( i think, if not not all your drano will dissolve) so it should be about five times the energy released compared to just two grams.
796425
calorimeters.........or bomb calorimeters
812576
From the reaction you had heat produced\n\nQ=m*Cp*ΔT\n\nfor water Cp= 1 calorie/(gram*Celsius)\n\nYou have a total of 50+50 =100mL and since d=1.00 g/mL you have 100 g\n\nso Q =100*1*(31.43-25.32) = 611 cal\n\nyou mixed mole HCl= C*V= 1*0.05= 0.05 with\nmole NaOH =C*V =1.1*0.05 =0.055 which means that, since the stoichiometry of the reaction is 1:1, HCl is the limiting reagent\n\n0.05 mole HCl give 611 cal\n1 mole HCl gives x\nx=611/0.05= 12220 cal/mole =12.22 Kcal/mole
821448
maybe forming an MgI2
518561
Mg(OH)2 n then Al(OH)3 gel
954561
Trying to make nitroglycerin, eh?\n\nWon't find out how to do it from me.  And beware of some of the other sources out there -- they're deliberately miswritten so that you'll blow yourself up.