name the catalyst used in solvay process?
829049
Ammonia (NH3) is the catalyst. Are u in 10th class?
1172999
1) exothermic reaction gives off heat\n2) a catalyst speeds up a rxn\n3) chemical reaction\n4) 1  + 4 --> 1 + 1 + 2\n\ncoefficiant of HCl is one
813911
HBr ---> H(+) + Br(-)\nH2SO3 ---> H(+) + HSO3(-)\nCH3-COOH ---> H(+) + CH3-COO(-)
1175500
catalyst :- substance which increase the rate of reactoin without being get consumed in it.\nenzyme :- boilogical catalyst which increase the rate of boilogical reaction \n                  e.g.    amaylase enzyme found in human saliva\nsacrificial protection :- reduction of corrosion of a metal in an electrolyte by galvanically coupling it to a more anodic metal\n\n\n\nvisit for more infor mation on corrsion\n\n\nwww.corrosionsource.com/handbook/glossary
881597
Cr2(SO4)3 + 6KOH  --> 2Cr(OH)3 + 3K2SO4
575918
0, they are reaction catalysts
952998
The reductive dissolution of goethite ( -FeOOH) and hematite ( -Fe 2 O 3 ) by phenolic reductants has been examined in order to improve the understanding of iron transformations in soils, sediments and aquifers. Rates of goethite reductive dissolution by hydroquinone increased as the pH was increased from pH 1.8 to 4.65, arid the following reaction stoichiometry was obeyed: 2 - FeOOH + QH 2 = 2 Fe 2+ + Q + 4 OH - . As the pH was increased from pH 4.5 to 6.0, the reductive dissolution rate decreased to below the detection limit. At pH 3.4, the reductive dissolution of hematite was two orders of magnitude slower than goethite. The relationship between structure and reactivity was examined for a series of mono-, di-, and tri-hydroxybenzene reductants. Rates of reductive dissolution decreased in the following order: catechol ~- hydroquinone 〉 3,4-dihydroxybenzoic acid 〉 resorcinol-phenol-4-hydroxybenzoic acid.
290781
MgSO4(s) + 2HCL(aq) ---> H2SO4(aq) + MgCl2 (aq)
377199
B.  A catalyst speeds up the reaction, as said in the question.  It's mostly just narrowing it down.  Obviously it provides a lower energy pathway if it speeds the reaction up, so it's not C or D.  It's not A, obviously.  Why would you want something that speeds the back reaction from products to reactants up? Well, unless specifically looking for it, I guess.   \nSo, B.
871578
http://www.olysun.com/Chem_121/Soln.html\n\n\ncc
222617
HCL is definitly not a catalyst cos it is very reactive. it can react with the acetic anhydride  to produce acetyl chloride.\nremember catalyst should nt undergo chemical reactions.
170129
CuSO4 (s)  --H2O-->  Cu+2 (aq) + SO4-2 (aq)
900424
The can be made of many other metals.  The question is how they work compared to the precious metal catalysts.  The reference shows one that contains cerium and copper.  Do a web search for "NOx and catalyst" and you will get a large bunch of references.
430714
the net effect on the catalyst is none, however to say that the catalyst does not interfere with the reactants is rubbish.  in many catalsyed reactions NO reaction will occur WITHOUT the presence of the catalyst.  \n\nPalladium coupling reactions (Heck, Sonogashira, Negishi, Suzuki etc) rely on the palldium catalyst OXIDATIVELY ADDING to the electrophilic reagent, typically an aryl/heteroaryl halide.  Depending on which catalyst you use it may lose two of its own ligands, such as will happen with Pd(PPh3)4, and formally form bonds with the aryl/heteroaryl bromide.\n\nIn hydrogenations, the hydrogen is temporarily absorbed on to the Pd/C.  Without this catalyst no reaction will happen.\n\nFor alkene metathesis reactions, Grubbs catalyst, and variations thereof, RELY on the formation of Ru=C bond, for the reaction to occur.  The Ru from the catalyst and the C from your terminal alkene.\n\nIn many reactions the the actual catalyst is an unstable species in itself.  For cross-coupling reactions you may use Pd(PPh3)4, PdCl2(PPh3)2 etc etc, however the catalytic species is "Pd(PPh3)2" - this has 14 electrons as opposed to the former which are more stable with 18 electrons.  It is this highly reactive "Pd(PPh3)2" species which is looking for extra electrons to stabilise it.\n\nUltimately without going into more detail, in many chemical reactions the catalyst DOES react with the other components in a chemical reaction - it HAS to.\n\nIt is correct that the catalyst has this effect because it provides the reagents with an alternative pathway, with a lower activation energy.\n\nBecause you are forming an unstable species in the active catalyst it is not always possible to recover the catalyst.  It's similar to a battery running down over time.\n\nMany industrial processes however do spend time recovering all the metals and regenerating the catalyst as they are often very expensive.
677341
The reaction is\n\nH2O2(aq) + 3I-(aq) + 2 H+(aq) I3-(aq) + 2 H2O(aq)\n\nThe reaction above is often very slow, so a catalyst is usually added. Ammonium molybdate works; so do other transition metal ions. The catalytic action probably involves a free radical mechanism. Hydrogen peroxide can reduce MnO4-, but molybdate isn't a strong enough oxidizing agent to be reduced.
817601
try the local chemist....
1049433
http://genchem.chem.wisc.edu/sstutorial/FunChem.htm