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INDIVIDUAL WORK-2
For students all specialities
MODUL 2
In the maximal possible exited state the total spin of an atom makes 3. Find the number of the group, in which located this atom: | |
a | 2 |
b | |
c | |
d | |
f |
Among the given electronic configurations the smallest value of energy of ionization corresponds to: | |
a | 1 s 22 s 22 p 3 |
b | 1 s 22 s 22 p 63 s 2 |
c | 1 s 22 s 22 p 6 |
d | 1 s 22 s 22 p 63 s 1 |
The reason of periodic change of properties of elements is: | |
a | Increase of a charge of a nucleus of atom |
b | Increase of radius of atoms in groups |
c | Periodic repetition of similar electronic structures |
d | Increase of number of electrons in atoms |
At interaction of 1,5 g of an oxide of alkaline metal with water was formed 1,65 g of an alkaline. This metal is: | |
a | Lithium |
b | Potassium |
c | Sodium |
d | Cesium |
f | Rubidium |
Mass of 1l of an hydrogen compound of an element, which is in the seventh group of periodic system, under normal conditions is 1,63 l. This element is: | |
a | Bromine |
b | Astatium |
c | Fluorine |
d | Iodine |
f | Chlorine |
| |
At the decomposition of 25 g of a carbonate of twovalent metal was liberated 5,6 l carbon dioxide under normal conditions. The formula of the salt looks like: | |
a | SrCO3 |
b | CaCO3 |
c | MgCO3 |
d | BeCO3 |
f | BaCO3 |
Find covalence and oxidation state of sulphur in a molecule Н2S: | |
a | 3, +2 |
b | 6, +2 |
c | 4, –2 |
d | 6, –2 |
f | 2, –2 |
Find charge of the complex ione, charge and coordination number of the central atom in complex compound K4[Fe(CN)6]: | |
a | 4–, 2+, 4 |
b | 2–, 6+, 4 |
c | 3–, 3+, 3 |
d | 4–, 2+, 6 |
f | 2–, 3+, 6 |
Find concentration of complex ion [Co(NH3)5]3+, that forms according the first step of dissociation (first instability constant is К1 = 4×10–5) in 0,01 M solution of hexaamminecobalt (ІІІ) chloride, if concentration of complex ion [Co(NH3)6]3+ at its dissociation practically does not change: | |
a | mol/ |
b | 4×10–5×0,01 mol/ |
c | 0,01 mol/ |
d | mol/ |
f | mol/ |
Thermochemical equations of formation of nitrogen and carbon oxides look like: 1/2N2(g)+ 1/2O2(g)= NO(g), DНо = 90,25 kJ; С(crist)+ 1/2O2(g)= СО(g), DНо = –110,5 kJ. It means, that in this reactions: | |
a | 200,75 kJ of heat is liberated |
b | 90,25 kJ is absorbed and 110,5 kJ of heat is absorbed |
c | 90,25 kJ is absorbed and 110,5 kJ of heat is liberated |
d | 200,75 kJ of heat is absorbed |
f | 90,25 kJ is liberated and 110,5 kJ of heat is absorbed |
The rate constant of chemical reaction 2SO2+ O2= 2SO3 is 1,6. Initial concentrations of oxygen and oxide of sulfur are 0,16 mol/l and 1,2 mol/l accordingly. After some time the concentration of oxygen has decreased down to 0,06 mol/l. Find thus the concentration of sulfur (IV) oxide and the reaction rate: | |
a | С(SО2) = 1,0 mol/l; 9,6×10–2mol/l×s |
b | С(SО2) = 0,12 mol/l; 1,76×10–5mol/l×s |
c | С(SО2) = 1,1 mol/l; 3,46×10–3mol/l×s |
d | С(SО2) = 1,14 mol/l; 2,56×10–3mol/l×s |
f | С(SО2) = 0,08 mol/l; 9,84×10–4mol/l×s |
Equilibrium of reaction H2+ Cl2= 2НСl(g) was established at the following concentrations of substances: [Н2] = 0,25 mol/l; [Cl2] = 0,05 mol/l; [НСl] = 0,9 mol/l. Find the initial concentration of chlorine: | |
a | 0,7 mol/l |
b | 0,5 mol/l |
c | 0,8 mol/l |
d | 0,2 mol/l |
f | 0,6 mol/l |
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