Values are resulted in the table:

Substance
ZnCl2	–478,2
CuCl2	–262,3

1. -215,9

2. 740,5

3. –903,6

4. 904,2

5. 370,2

177. What quantity of warmth will be allocated at dissolution of 200 g. copper oxide in hydrochloric acid at the thermo chemical reaction: CuO+2HCl = CuCl₂+H₂O - 63, 6 kJ.?

1. 160

2. 140

3. 120

4. 180

5. 110

178. To calculate quantity of warmth this will be absorbed at receiving of 12 g. of oxygen at the thermo chemical reaction: 2KNO₃= 2KNO₂+O₂+ 255 kJ.

1. 95,6

2. 80,4

3. 75,6

4. 69,6

5. 59,6

179. What quantity of warmth will be allocated at combustion of 4, 48 l. (n.c.) methane at the thermo chemical reaction:

CH₄+2O₂ = CO₂+2H₂O-878 kJ?

1. 175,6

2. 150,3

3. 140,6

4. 130,6

5. 165,3

180. Indicate condition parameters:

1. U,H

2. U,Q

3. Q,A

4. P,W

5. A,S

181. Thermal effect at formation of one mole of substance is called as warmth …

1. Formations

2. Combustion

3. Thermal effect

4. Dissolution

5. Crystallisation

182. Criterion of course of chemical process at entropy and volume constancy is

1. U;

2. H;

3. G;

4. A;

5. S;

183. Criterion of direction of chemical process at P=const, S=const is …

1. H;

2. A;

3. G;

4. U;

5. S;

184. Criterion of direction of chemical process at V=const, T=const is …

1. A;

2. U;

3. S;

4. G;

5. H;

185. At what values of thermodynamic potentials process goes spontaneously:

1. ΔG<0

2. ΔG>0

3. ΔH>0

4. ΔH<0

5. ΔA>0

186. Criterion of direction of chemical process at P=const, T=const is …

1. G;

2. A;

3. U;

4. S;

5. H

187. Energy of Gibbs in spontaneous process …

1. Decreases;

2. Increases;

3. Remains on the same place;

4. All answers are correct;

5. All answers are not correct;

188. Indicate changes of Gibbs's energy:

1. G=H-TS;

2. G=-HTS;

3. G=H+TS;

4. G=H-U;

5. G=H / TS;

189. Mendeleyev-Klayperon equation for 1 mole ideal gas:

190. Sedimentation, colour changing at adding of electrolyte to colloid are signs …

A) Coagulation;

B) Flocculation;

C) Stabilization;

D) Dialysis;

E) Osmosis

191. Passing through disperse system, light is absorbed, reflected or dissipated by particles. Dispersion of light most typical for systems …

1. colloid;

2. harddispers;

3. molecular;

4. ionic;

5. macroheterogeneous.

192. A coagulation rule: among organic ions coagulate action increases with increase... abilities.

1. sorb;

2. diffuse;

3. absorb;

4. electro kinetic;

5. electro foretic

193. The dispersive environment - gas, a disperse phase - a liquid.

1. Fog;

2. emulsion;

3. suspension;

4. solid sol;

5. smoke;

194. The dispersive environment - gas, a disperse phase – solid substance.

1. smoke

2. solid sol;

3. solid foam

4. suspension

5. fog

195. The dispersive environment - liquid, a disperse phase - a liquid.

1. emulsion ;

2. sol;

3. fog;

4. smoke;

5. suspension;

196. The dispersive environment - liquid, a disperse phase - solid substance.

1. suspension;

2. smoke;

3. dust;

4. fog;

5. emulsion;

197. The dispersive environment -solid, a disperse phase - solid.

1. solid sol;

2. suspension;

3. smoke;

4. dust;

5. fog;

198. The dispersive environment - liquid, a disperse phase - solid.

1. without name;

2. sol;

3. smoke;

4. D)fog;

5. E)suspension;

199. The dispersive environment - gas, a disperse phase - liquid.

1. without name;

2. fog;

3. smoke;

4. dust;

5. sol;

200. The dispersive environment - solid, a disperse phase - gas.

1. solid foam;

2. smoke;

3. dust;

4. fog;

5. suspension;

201. The dispersive environment - liquid, a disperse phase - gas.

1. foam ;

2. smoke;

3. dust;

4. fog;

5. sol;

202. Faraday and Tindal have described the phenomenon observed at missing of light through colloid solution, named...

1. Opalescence,

2. Extinction,

3. Diffraction,

4. Reflexion ,

5. Absorption

203. Faraday and Tindal have described the phenomenon observed at missing of light through colloid solution, named...

1. Opalescence,

2. Extinction,

3. Diffraction,

4. Reflexion ,

5. Absorption

204. The system consisting of several phases is called:

1. Heterogeneous,

2. homogeneous,

3. uniform,

4. phase, u

5. nicomponent

205. The solid substance on which surface there is an adsorption, is …

1. adsorbent;

2. adsorbate;

3. adsorbtive;

4. sorbat;

5. sorbent;

206. Spontaneous transition of substance from volume of environment in a phase is named...

1. Adsorption;

2. hemosorption;

3. desorption;

4. sorption;

5. Absorption;

207. Absorption of substance from the environment by volume of a phase of disperse system name …

1. Absorption,

2. Adsorption,

3. hemosorption,

4. desorption,

5. sorption

208. Unilateral diffusion of the dispersive environment in porous systems is called:

1. osmosis,

2. electrophoresis,

3. Dialysis,

4. electroocmosis,

5. Electrodialysis.

209. Directed moving of particles of disperse phase under the influence of the enclosed potential difference.

1. Electrophoresis;

2. Electrodialysis,

3. Electroosmosis;

4. Dialysis;

5. Electrolysis

210. The phenomena of electrophoresis and electroosmosis is ... in a science and the technician.

1. Useful,

2. Harmful,

3. Indifferent,

4. Negative,

5. useless

211 The general formula of alkanes

A) C_nH_2n+2

В) C_nH_2n

С) C_nH_2n-2

D) C_nH_2n-6

Е) C_nH_2n-4

212 The general formula of alkenes

A) C_nH_2n

В) C_nH_2n+2

С) C_nH_2n-2

D) C_nH_2n-6

Е)C_nH_2n-4

213 The general formula of alkadienes

A) C_nH_2n-2

В) C_nH_2n-6

С) C_nH_2n

D) C_nH_2n-4

Е) C_nH_2n+2

214. The general formula of alkynes

A) C_nH_2n-2

В) C_nH_2n-6

С) C_nH_2n

D) C_nH_2n-4

Е) C_nH_2n+2

215. Indicate alkanes: 1) С₆Н₁₂ 2) С₅Н₁₂ 3) С₄Н₁₀ 4) С₂Н₂ 5) С₄Н₈

A) 2,3

В) 1,2

С) 3,4

D) 4,5

Е) 1,5

216. Indicate alkenes: 1) С₃Н₈ 2) С₄Н₈ 3) С₄Н₁₀ 4) С₅Н₁₀ 5) С₂Н₂

A) 2,4

В) 1,5

С) 2,3

D) 1,3

Е) 4,5

217. Indicate alkynes: 1) С₃Н₄ 2) С₆Н₁₂ 3) С₅Н₁₀ 4) С₄Н₆ 5) С₄Н₈

A) 1,4

В) 2,3

С) 1,2

D) 2,5

Е) 3,5

218. Determine the class of the compound: СН₃ - CH₂ - CН₂ - CH₂ - OH

A) alcohol

В) ester

С) ketone

D) aldehyde

Е) ether

219. Determine the class of the compound: СН₃  CH₂  О  CН₂  CН₃

A) ether

В) ester

С) ketone

D) aldehyde

Е) alcohol

220. Determine the class of the compound:

A) ketone

В) acid

С) ester

D) aldehyde

Е) ether

221. Determine the class of the compound: СН₃  CH₂  CН₂  CН₂ COOH

A) carboxylic acid

В) ester

С) ketone

D) aldehyde

Е) alcohol

222. Determine the type of reaction:

A) substitution

В) addition

С) decomposition

D) oxidation

Е) reduction

223. Determine the type of reaction:

A) substitution

В) addition

С) decomposition

D) oxidation

Е) reduction

224. Determine the type of reaction:

A) addition

В) substitution

С) decomposition

D) oxidation

Е) reduction

225. Determine the type of reaction: СН₃  СH = CH  СН₃ + H₂O 

A) addition

В) substitution

С) decomposition

D) oxidation

Е) reduction

226. Alkane with octane number 0

A) heptane

В) octane

С) hexane

D) propane

Е) pentane

227. Alkane with octane number 100

A) 2,2,4-trimethylpentane

В) octane

С) hexane

D) heptane

Е) pentane

228. Reagents interacting with alkanes:

1. Cl₂(hn) 2. HNO₃+H₂O 3.NaOH 4. Br₂ +HOH 5. HOH

A) 1,2

В) 4,5

С) 3,4

D) 3,5

Е) 1,4

229. Reagents interacting with alkanes:

1.NaOH 2. Br₂ +HOH 3. HOH 4. Cl₂(hn) 5. HNO₃+H₂O

A) 4,5

В) 1,2

С) 3,4

D) 3,5

Е) 1,4

230. Reaction condition for nitration of alkanes:

A) HNO₃ diluted

В) HNO₃ concentrated

С) HNO₃+ H₂SO₄

D) NO₂

Е) N₂O₄

231. HNO₃ (diluted) is used for …

A) nitration of alkanes

В) oxidation of alkanes

С) decomposition of alkanes

D) conversion of alkanes

Е) radical substitution

232. Bromic water is decoloured by compounds:

1) alkenes 2) alkanes 3) dienes 4) alcohols

A) 1,3

В)1,2

С) 2,3

D) 3,4

Е) 2,4

233. Bromic water is decoloured by compounds:

1) alkenes 2) alkanes 3) dienes 4) alcohols

A) 1,3

В)1,2

С) 2,3

D) 3,4

Е) 2,4

234. Name the final product:

A) acetylene

В) ethylene

С) ethane

D) propyne

Е) propylene

235. The author of nitrate reaction for alkanes:

A) Konovalov

В) Kolber

С) Zaitsev

D) Wurtz

Е) Butlerov

236. Synthetic high-molecular substances:

Polyethylene;

Rubber;

Fibers;

Nucleinic acids;

polysaccharide

237. Electronegativity is an ability of atom...

A) to attract electrons

B) to delocalized electrons

C) to distribute electrons

D) to give electrons

E) to push away electrons

238. Characteristic of covalence bond

A) Polarizability

B) Length of bond

C) Electronic density

D) Hardness of bond

E) Electro negativity

239. Specify, what sublevel is filled after 4s

А) 3d

В) 4p

С) 3S

D) 5S

Е) 4f

240. Specify the number of electrons in atom of aluminum

А) 13

В) 27

С) 14

D) 11

Е) 10

241. What of metals refers to d - elements?

А) Fe

В) Na

С) Ca

D) Ba

Е) Li

242. Specify the number of electrons of oxygen atom

А) 8

В) 16

С) 32

D) 2

Е) 18

243. What formula reflects the total number of electrons in energy level?

А) N=2n²

В) N=2n

С) N=n

D) N= √2n

Е) N=2√n

244. Name the element that has an electronic formula...3s²3p³

А) P

В) Al

С) O

D) S

E) K

245. In what group are alkaline metals in D.I.Mendeleyev table located?

А) I A

В) II A

С) III A

D) VI A

Е) VII A

246. In what group is alkaline earth metals are located in the table of D.I.Mendeleyev?

А) II A

В) I A

С) III A

D) VII A

Е) VIII A

247. In what group are halogens in D.I.Mendeleyev's table located?

А) VI A

В) VII A

С) I A

D) II A

Н) VII A

248. Specify the number of neutrons for an atom of potassium

А) 20

В) 19

С) 39

D) 21

Е) 5

249. What electronic formula corresponds to atom of oxygen?

А) 1S²2S²2p⁴

В) 1S²2S²2p³

С) 1S²2S²2p⁵

D) 1S²2p⁶

Е) 1S²2S²2p¹

250. Specify the maximum amount of electrons at the first energy level

А) 2

В) 18

С) 8

D) 32

Е) 38

251. Number of the electrons on the outer energy p-sublevel of atom of chlorine is equal to

А) 5

В) 7

С) 3

D) 6

Е) 1

252. How many power levels has the atom with a serial number 8

А) 3

В) 1

С) 2

D) 4

Е) 8

253. Specify the maximum number of electrons on p-orbital

А) 6

В) 8

С) 2

D) 10

E) 5

254. How many elements in the fourth period of periodic system?

1. 18

2. 10

3. 22

4. 32

5. 8

255. What the line of elements is presented in increasing order of nuclear radius?

1. О, S, Se, Те

2. С, N, О, F

3. Na, Mg, Al, Si

4. J, Br, Се, F

5. He, В, Xe, Кr

256. How many of energy orbitals exist for chemical elements?

6. 4

7. 3

8. 2

9. 5

10. 6

257. What is the electronic formula of Al

А) 1S²2S²2p⁶3S²3p¹

В) 1S²2S²2p⁶3S₂3p³

С) 1S²2S²2p⁶3S²3p⁶

D) 1S²2S²2p⁶3S²3p⁰

Е) 1S²2S²2p⁶3S¹

258. What sublevel is filled after 4S

А) 3d

В) 4p

С) 3p

D) 4d

Е) 4f

259. What sublevel is filled in atoms after the sublevel 5s?

А) 4d

В) 4p

С) 4f

D) 5p

Е) 6s

260. The electronic formula of atom is 1S²2S²2p⁶3S²3p⁶4S²3d⁶ . What element is it?

А) Fe

В) Mn

С) Ca

D) Ni

Е) Pb

261. What maximum number of electrons could the atom contain in an electronic level n=4

А) 32

В) 2

С) 8

D) 18

Е) 6

262. Indicate the simple substances: O₂, , , , С₂Н₂, Н₂O₂, H₂S, H₂SO₄, NaCI

1. 

2. ,

3. 

4. ,

5. 

263. Types of chemical reactions according to the mechanism of interaction

1. neutralizations, redox reactions, precipitations, complexations

2. connections, decompositions, replacements, exchanges

3. convertible and irreversible

4. direct and return

5. exothermic and endothermic

264. The basis of the neutralization is the reaction:

1. Н ⁺ + OH^- → Н₂О

2. Ва^{2 +} + СО₃^2- → ВаСО₃

3. Вr₂ + 2е → 2Br^--

4. Cu^{2 +} + 2OH^- → Cu (OH) ₂

5. Ag ⁺ + CI^- → AgCI

265. What element forms amphoteric oxides?

А) Al

В) Na

С) Ca

D) Mg

Е) Ba

266. Specify amphoteric oxides

А) Al₂O₃;ZnO

В) CuO;Na₂O

С) ZnO;CO₂

D) Na₂O;Fe₂O₃

Е) FeO;P₂O5

267. Specify the acid oxides

А) CO₂;P₂O₅

В) CaO;SO₃

С) P₂O₅;Fe₂O₃

D) Al₂O₃;K₂O

Е) ZnO;CrO₃

268. Specify not salt-forming oxides

А) CO; NO

В) CO₂; SO₃

С) N₂O; P₂O₅

D) Na₂O; SiO

Е) SO₃; SO

269. To define the base oxides ВеО,

1. ,

2. ВеО, ,

3. ВеО,

4. ВеО,

5. 

270. To define the acidic oxides: Na₂O, СоО, F , MnO₂, BaO, S , Si

1. SO_2, SiO₂,

2. Na₂O, BaO,

3. CoO, SO₂,

4. MnO₂, Na₂O ,

5. СоО, BaO

271. To define the one-basic acids: Н₃РO₄, HCI, H₂MnО₄

1. 

2. 

3. 

4. 

5. 

272. To define the two-basic acids:

1. ,

2. 

3. 

4. 

5. 

273. To define the three-basic acids: , H₃PО₄, ,

1. , H₃PО₄

2. 

3. HJ,

4. H₃PО_4,

5. 

274. Specify strong acid:

1. 1

2. 5

3. 2

4. 3

5. 4

275. Specify strong acids: H₂S0₄, H₂S, HJ, H₂SО₃. HCN, H₂C , HCI

1. H₂SО_4, HJ, HCI

2. H₂S, H₂C , H₂SО₄

3. HJ, HCN, H₂C ,

4. H₂SО₃, H₂S, HJ

5. H₂SО_4, HCN, HCl

276. Specify weak acids: CH₃COOH, НСlO₃, H₂CO₃, HN O₂, HBr, HJ, НClO₄

1. C COOH, C , HNО₂

2. HCI . HCI . HN

3. C COOH, HBr, HJ

4. C , HJ, НClO₃

5. НClO₄, HN , C COOH

277. The strongest oxygen containing chlorine acid:

1. HCl

2. HCl

3. HClO

4. HCl

5. HCl

278. What hydroxides shows amphoteric character

А) Al(OH)₃

В) NaOH

С) Ca(OH)₂

D) Mg(OH)₂

Е) KOH

279. Define oxidation degree of nitrogen: N N₂H₄, NH₂OH

1. -3,-2,-I

2. 2; I; 3

3. -l,+2,+3

4. 0, +2, -3

5. -2,-1,0

280. Define oxidation degree of sulfur: SО₂, H₂S, Na₂SО₃, CS₂, H₂SО₄

1. +4,-2, +4, +4, +6

2. +2,-4, +2,-4,-4

3. +2,-2, +4, -4,+6

4. +2,-2,-4,+4, -6

5. +4, +2,-4,+2,-4

281. Define oxidation degree of Мn: МnО,

1. +2, +4, +3,+7

2. +2, -2, +4, +6

3. -2, +2,-4,+7

4. +2,-4,+4, -7

5. +2, +4, -6, -7

282. In what compounds nitrogen has oxidation degree +5

1. 

2. 

4. 

5. 

283. In what compounds chromium has oxidation degree +6

1) ;2) С Оз; 3) Na 4) 5) Cr ; 6)

1. 1,5

2. 3,5

3. 4,6

4. 1,2

5. 5,4

284. In what compounds manganese has oxidation degree +7

1. 

2. 

3. 

4. 

5. 

285. Characteristic degree of oxidation for copper: +1, +2, +3, +4, +6

1. +2

2. +4

3. +3

4. +1

5. +5

286. Maximum degree of oxidation for nitrogen

А) +5

В) +3

С) +1

D) 0

Е) +6

289. Define the degree of oxidation of bromine in bromide of potassium

А) -1)

B) +1

С) +7

D) +5

E) -3

290. Define the degree of oxidation of sulphur in Na₂SO₄

А) +6

В) -6

С) +4

D) -4

Е) 2

291. The charge of the proton is equal to

А) +1

В) 0

С) -1

D) 1,6

Е) 6,02×10²³

292. Specify metal with valence 3

А) Al

В) Ca

С) Mg

D) Ag

Е) Zn

293. Specify the chloride-ion

А) Cl^-

B) Cl^2-

С) Cl⁰₂

D) Cl^4-

E) ClO^-₄

294. Specify sulfate - ion

А) SO^2-₄

В) SO^-₄

С) SO^3-₄

D) HSO^2-₄

Е) HS^-

295. To define coordination numbers of forming complexes in compounds: K ,

1. 2, 6, 6

2. 1, 4, 3

3. 1, 5, 3

4. 0, 3, 3

5. 1, 4, 3

296. To define a charge of forming complex in compound

1. +2, +3

2. +1, +2

3. +1, -1

4. +2, +5

5. +1, +6

297. What is the type of reaction H₂SO₄+ 2NaOH =Na₂SO₄+ 2Н₂O:

I) neutralization; 2) replacement; 3) decomposition; 4) addition; 5) oxidation-reduction?

1. 1

2. 3

3. 4

4. 2

5. 5

298. What reactions belong to the oxidation-reduction?

2. ;

3. ;

4. Fe+S=FeS

1. 2, 4

2. 1, 3

3. 2, 3

4. 1, 4

5. 2, 1

299. What is the type of reaction: ?

1. Disproportion

2. Neutralization

3. Precipitate

4. Decomposition

5. Exchange

300. Oxidizer:

Accepts electrons;

Gives electrons;

Replaces protons;

Reduces enthalpy;

Absorbs warmth.

301. Reducer:

1. Gives electrons;

2. Accepts electrons;

3. Replaces protons;

4. Reduces enthalpy;

5. Absorbs warmth.

302. Oxidizer for the given reaction:

1. ,

2. ,

3. ,

4. ,

5. 

303. Reducer for the given reaction: 4NH₃+3O₂=2N₂+6H₂O

1. N^-3

2. H⁺¹

3. O⁰

4. N⁰

5. O^-2

304. To specify the sum of coefficients for reaction:

1. 10

2. 8

3. 6

4. 2

5. 4

305. To specify the sum of coefficients for reaction:

А)20

Б)12

В)10

Г)14

Д)11

306. To specify the sum of coefficients for reaction: K₂S +K₂Cr₂ +H₂SО₄  S + K₂S0₄ + Cr₂ (SО₄ +

А) 26

Б) 20

В) 24

Г) 18

Д)22

307. To specify the sum of coefficients for reaction: +

A.7

B.8

C.6

D.5

E.3

308. To specify the sum of coefficients for reaction:

1. 13

2. 10

3. 9

4. 7

5. 14

309. To specify the sum of coefficients for reaction:

1. 19

2. 17

3. 14

4. 21

5. 13

310. To specify the sum of coefficients for reaction:

1. 7

2. 6

3. 4

4. 8

5. 5

311. To specify the sum of coefficients for reaction:

1. 22

2. 20

3. 18

4. 16

5. 14

312. To specify the sum of coefficients for reaction: →

1. 10

2. 8

3. 6

4. 4

5. 5

313. To specify the sum of coefficients for reaction: + + →Cr + + O

A) 14

B) 12

C) 10

D) 8

E) 6

314. pH of solution calculates according to the formula:

1. pH = 14 - pOH

2. pH = 14 + pOH

3. pH = K_gC + 10

4. pH = N/n

5. pH = n/N

315. The hydroxyl indicator of environment is equal:

1. pH = [H⁺][OH^-]

2. рОН = -lg[H⁺]

3. [pОH = - lg[ОH^-]

4. H₂O] = -lg[OH^-]

5. pOH= -lg[H⁺][OH^-]

316. To specify an alkaline solution:

1. [H⁺] = 10^-12

2. [H⁺] = 10^-7

3. [ОH^-] = 10³¹

4. [ОH^-] = 10^-3

5. [H ₂О] = 10⁷

317. To specify a neutral solution:

1. H⁺] = [OH^-]

2. [H⁺] > [OH^-]

3. [H⁺] < [OH^-]

4. pH = 12

5. pH = 17

318. Electrolysis is:

1. oxidation-reduction process;

2. disintegration of a molecule of electrolit to ions;

3. process of association of ions;

4. movement of electrons around of nucleus;

5. process of molecule dissociation.

319. Cathode is an electrode at which there is a process:

1. Reduction of cations;

2. Oxidation of anions;

3. Disintegration of molecules;

4. Association of ions;

5. Changing of oxidation degree of an element.

320. Anode is an electrode at which there is a process:

1. Oxidation of anions;

2. Reduction of cations;

3. Disintegration of molecules;

4. Association of ions;

5. Changing of oxidation degree of an element.

321. Electrolyte of the lead accumulator is the solution of:

1. H₂SO₄

2. H₂O

3. H₃PO₄

4. HF

5. HCI

322. Inhibitor is:

diminish of corrosion

corrosion accelerator

protector

accumulator

galvanic cell.

323. Faraday number is equal:

1. 96500

2. 73500

3. 760

4. 101

5. 83100

324. Potential of a standard hydrogen electrode is equal:

1. 0

2. 1

3. 2

4. 5

5. 9

325. To inert anodes belong:

1. graphite, platinum

2. zinc, copper

3. chrome, manganese

4. zinc, chrome

5. iron, zinc

326. To active anodes belong:

1. copper

2. platinum

3. neon

4. graphite

5. plastic

327. At electrolysis of NaCl solution at the anode it is allocated:

1. chlorine

2. sodium

3. oxygen

4. hydrogen

5. water