Option 1
1. Complete the equations of the reactions:
Ba + S →
KCl(solid)+ H2SO4 (solid)→
NaI + Cl2 →
H2S + O2 (ext.)→
SO2 + NaOH (natural)→
2. Carry out the transformations according to the scheme:
Cl2 → HCl → FeCl2 → FeCl3 → NaCl → AgCl
3. With which of the following substances will dilute sulfuric acid react: zinc, sodium sulfate, potassium sulfite, carbon oxide (4), mercury oxide (2), barium hydroxide, magnesium chloride, silver? Give equations of possible reactions and state their type.
4. Write down the equation for the reaction of concentrated sulfuric acid with magnesium. Determine the oxidation states of the elements, make an electron balance diagram and set up the coefficients.
5. What volume of hydrogen (n.y.) will be released when magnesium is dissolved in 60 grams of 3% hydrochloric acid solution?
Test work №2 on the topic: Halogens. Oxygen and sulfur.
Option 2
1. Complete the equations of the reactions:
H2+ S →
K2SO4+ Ba(OH)2→
CaBr2 + Cl2 →
H2S + CuSO4 →
CuCl2 + Fe →
2. Carry out transformations according to the scheme:
S →FeS → H2S → SO2 → Na2SO3 → SO2
3. Which of the following substances will hydrochloric acid react with: iron, sodium sulfate, potassium carbonate, barium oxide, mercury, copper (2) hydroxide, calcium chloride, silver? Give equations of possible reactions and state their type.
4. Write down the equation for the reaction between concentrated sulfuric acid and mercury. Determine the oxidation states of the elements, make an electron balance diagram and set up the coefficients.
5. What volume of hydrogen (n.y.) will be released when magnesium is dissolved in 60 grams of 3% hydrochloric acid solution?
Option 3
1. Complete the equations of the reactions:
Na + Br2 →
CaCl2 (solid) + H2SO4 (solid) →
KI + Br2 →
H2S + O2(incomplete)→
H2SO4( elect) + KOH →
2. Carry out the transformations according to the scheme:
S → SO2 → CaSO3 → SO2 → SO3 → H2SO4
3. With which of the following substances will hydrochloric acid react: silver, sodium hydroxide, potassium sulfite, sulfur oxide (4), iron oxide (2), silver nitrate, magnesium chloride, aluminum? Give equations of possible reactions and state their type.
4. Write down the equation for the reaction of concentrated sulfuric acid with nickel. Determine the oxidation states of the elements, make an electron balance diagram and set up the coefficients.
5. What is the mass of the precipitate formed by the interaction of 800 grams of a 15.6% solution of sodium sulfide with lead nitrate?
Test work №2 on the topic: Halogens. Oxygen and sulfur.
Option 4
1. Complete the equations of the reactions:
Hg+ S →
CuSO4+ Fe→
HBr + Cl2 →
H2S + Pb(NO)3→
SO2 + O2→
2. Carry out the transformations according to the scheme:
MnO2 →Cl 2 →HCl → BaCl2 →HCl → HNO3
3. With which of the following substances will dilute sulfuric acid react: iron, sodium sulfate, potassium sulfide, lithium oxide, copper, mercury (2) hydroxide, zinc nitrate , silver? Give equations of possible reactions and indicate their type.
4. Write down the equation for the reaction of concentrated sulfuric acid with copper. Determine the oxidation states of the elements, make an electron balance diagram and set up the coefficients.
5. 2.24 liters of hydrogen sulfide were dissolved in 250 grams of water. What is the mass fraction of hydrogen sulfide in the solution obtained?
