MIDLE TEST OF SEMESTER 2
Education Year 2011/2012
Education Year 2011/2012
Subject : Chemistry
Class : X
Day, Date : xxxxx, March, 2012
Time allotment : 07.30 – 09.30 (120 minutes)
Class : X
Day, Date : xxxxx, March, 2012
Time allotment : 07.30 – 09.30 (120 minutes)
General Directions
1. Do this test of chemistry on the answer sheet that is provided.
2. Write your name and your serial number in the space provided.
3. The problems consist of 40 number of multiple choices and 5 number of essays
4. Read the instructions to do the problems
5. The maximum score of multiple choices is 40. The maximum score of essay is 30.
6. Work accurately
7. If you make a mistake in choosing of multiple choice answer, score out with double strikethrough ( ), and then put a cross ( X ) on the right answer
8. The calculator is allowed to used
9. Re-examine your work before hand in to supervisor
=0=
Special Directions
I. Multiple choices
Choose the correct answer by put a cross on A, B, C, D, or E in the answer sheet
1. Known Ar K = 39, Fe = 56, C = 12, N = 14. The relative formula mass (Mr) of K3[Fe (CN)6] is . . . .
a. 329 d. 1000
b. 792 e. 1210
c. 851
2. The molar mass (mm) of aluminum sulfate is ….
(Ar Al =27, S = 32, O = 16,)
a. 106 grams.mole−1
b. 180 grams.mole−1
c. 310 grams.mole−1
d. 342 grams.mole−1
e. 400 grams.mole−1
3. The relative atomic mass (Ar) of N = 14, O = 16, P = 31, S = 32, Cl = 35,5, K = 39, Fe = 56, Sn = 119, Ba = 137. Among the following substances, it has the biggest molar mass (mm) is ….
a. sulfur, S8 .
b. iron(II) sulfide, FeS
c. barium phosphate, Ba3(PO4)2
d. potassium sulfate, K2SO4
e. tin(IV) nitrate, Sn(NO3)4
4. The molar mass (mm) sodium carbonate, Na2CO3 is 106 g/mole.
The mass of 3.01 x 1024 molecules of Na2CO3 is ….
a. 212 g d. 530 g
b. 380 g e. 600 g
c. 424 g
5. The Iron element contains 3.01 x 1022 atoms of Fe. The moles amount of iron is ….
a. 0.01 mole
b. 0.05 mole
c. 0.50 mole
d. 1.50 moles
e. 5.00 moles
6. 400 mL of 90% alcohol solution by volume is diluted by adding 100 mL of water. The concentration of alcohol solution after being diluted is ….
a. 72% d. 60%
b. 70% e. 45 %
c. 65%
7. The composition of sugar and water in 300 g of 20 % sugar solution by mass is ….
a. 15 g of sugar and 285 g of water
b. 60 g of sugar and 240 g of water
c. 30 g of sugar and 270 g of water
d. 75 g of sugar and 225 g of water
e. 45 g of sugar and 255 g of water
8. In industrial area, mercury pollutes to the water. In the reality, from analyze 6 kg of water sample contain 24 mg of mercury. The content of mercury in the water in that industrial area is ….
a. 0.25 ppm d. 3.00 ppm
b. 0.50 ppm e. 4.00 ppm .
c. 1.50 ppm
9. In 250 mL of NaOH solution contain 6 grams of NaOH (mm NaOH = 40 g.mole−1 ). The concentration of NaOH solution is ….
a. 0.2 M d. 1.2 M
b. 0.6 M e. 1.5 M
c. 0.8 M
10. To make 200 mL of 0.25 M Fe2(SO4)3 solution, so the mass of Fe2(SO4)3 that is needed is …. (Ar Fe = 56, S = 32, O = 162
a. 20 g d. 60 g
b. 45 g e. 80 g
c. 50 g
11. 100 mL of 5 M NH4Cl solution is diluted by adding 100 mL of the water. The concentration of NH4Cl solution after being diluted is ….
a. 1.0 M d. 3.0 M
b. 1.5 M e. 3.5 M
c. 2.5 M
12. 100 mL of 6 M H2SO4 solution is diluted into 2 M by adding the water. The volume of adding of water is ….
a. 50 mL d. 150 mL
b. 200 mL e. 300 mL
c. 100 mL
13. In the compound of sulfuric acid, H2SO4, contains 16 grams of sulfur elements. (Ar H = 1, O = 16, S = 32) The mass of sulfuric acid is ....
a. 5.22 g d. 32 g
b. 8.0 g e. 49 g
c. 32 g
14. The mass of nitrogen that is contained in 12 grams of urea, CO(NH2)¬2, is ....
(Ar H = 1, C = 12, N = 14, O = 16)
a. 1.2 g d. 8.4 g
b. 2.8 g e. 11.2 g
c. 5.6 g
15. The mass of H2SO4 (mm = 98 g.mole−1 that is found in 400 mL of 0.25 M H2SO4 solution is ....
a. 0.49 gram d. 9.80 grams
b. 0.98 gram e. 12.40 grams
c. 4.90 grams
16. The number of molecules of CaCO3 that is contained in 50 grams of calcium carbonate is …. (Ar Ca = 40, C = 12, O = 16)
a. 1,204 x 1023 d. 9.03 x 1023
b. 3.01 x 1023 e. 1.204 x 1024
c. 6.02 x 1023
17. 4.6 g of the sample of a compound consist 2.8 g of nitrogen and 8.0 g of oxygen. The empirical formula of this compound is …. (Ar N = 14, O = 16)
a. NO d. N2O3
b. NO2 e. N2O5
c. N2O
18. The volume of 8.8 grams of CO2 (Mr = 44) that is measured at the room condition of pressure and temperature (RTP) is ….
a. 0.56 liter d. 4.8 liters
b. 0.88 liter e. 5.6 liters
c. 3.6 liters
19. The volume of 80 g of sulfur trioxide (Mr = 80) gas that is measured at temperature of 27 0C and pressure of 1 atmosphere is ….
a. 22.4 L d. 26.8 L
b. 24.0 L e. 28.2 L
c. 24.6 L
20. At the certain pressure and temperature, the mass of 1 L of X gas is 1.5 g.
At the same condition of pressure and temperature the mass of 10 L of nitrogen monoxide gas is 7.5 g. (Ar N = 14, O = 16)
The relative molecular mass (Mr) of X gas is ….
a. 33.6 c. 67.2 e. 80
b. 60 d. 78
21. The oxygen gas can be produced by decomposition of potassium chlorate KClO3, according to the reaction equation:
2 KClO3(s) 2 KCl(s) + 3 O2(g)
The mass of KClO3 (Mr = 122,5) that is needed to produce 6.72 liters of oxygen gas (STP) is .…
a. 86.75 grams d. 36.75 grams
b. 73.5 grams e. 55.13 grams
c. 24.5 grams
22. Ammonia gas can be made by reaction 53.5 grams of ammonium chloride (Mr NH4Cl =53.5) and sodium hydroxide according to the reaction as follow:
NH4Cl(s)+ NaOH(aq) NaCl(aq)+ H2O(l)+ NH3(g)
The ammonia gas that is produced to be measured at the certain (T.P) and at the same condition of (T.P) the mass of 5 L of CO2 (mm = 44 g.mole−1 gas is 11 g.
The volume ammonia gas is ....
a. 5 L d. 30 L
b. 10 L e. 40 L
c. 20 L
23. The completely burning of 6 grams of ethane gas, C2H6, produces carbon dioxide gas and water vapors, according to the reaction equation as follow:
2C2H6(g) + 7O2(g) 4 CO2(g) + 6H2O(g)
The volume carbon dioxide gas (STP) is …. (Ar C = 12, O = 16)
a. 2.24 L d. 8.96 L
b. 4.48 L e. 11.2 L
c. 5.60 L
24. The reaction of calcium carbide, CaC2, and water forms calcium hydroxide and acetylene gas, C2H2 according to the reaction as follow:.
CaC2(s) + H2O(l) Ca(OH)2(aq) + C2H2(g) (not balanced)
If 32 g of calcium carbide (Mr = 64) is reacted, so acetylene gas (STP) that produced is ....
a. 11.2 L d. 112 L
b. 22.4 L e. 224 L
c. 44.8 L
25. 27 grams of aluminum powder and 32 grams of sulfur powder is heated so that occur reaction to form aluminum sulfide. (Ar Al = 27, S = 32)
The reaction occurs as follow:
4 Al(s) + 6 S(s) 2 Al2S3(s)
In this reaction, reactant behave as the limiting reactant and the excessive reactant ….
a. sulfur is limiting reactant and there is aluminum excess of 2/3 moles
b. Aluminum is limiting reactant and there is sulfur excess of 1/2 mole
c. Aluminum is limiting reactant and there is sulfur excess of 1/3 mole
d. Aluminum is limiting reactant and there is sulfur excess of 2/3 moles
e. sulfur is limiting reactant and there is aluminum excess of 1/3 mol
26. Given a reaction:
3NaNO3(aq) + 5NaOH(aq) + 8Al(s) + 2H2O(l) 8NaAlO2(aq) + 3NH3(g)
In that reaction is mixed each of reactant is 10 moles. In that reaction a reactant behave as the limiting reactant is ….
a. NaNO3 d. H2O
b. NaOH e. NaNO3 dan H2O
c. Al
27. The following is reaction of formation of ammonia gas
N2(g) + H2(g) NH3(g)¬¬ (not balanced)
If the volume of nitrogen and hydrogen gas that is reacted each of them is 6 L, so the volume of ammonia gas produced is ….
a. 1 L d. 4 L
b. 2 L e. 5 L
c. 3 L
28. 100 mL of 1 M iron(III) nitrate solution is reacted with 200 mL of 2 M sodium hydroxide solution to form the precipitate of iron(III) hydroxide and sodium nitrate solution according to the following reaction equation:
Fe(NO3)3(aq) + 3NaOH(aq) Fe(OH)3(s) + 3NaNO3(aq)
The mass of precipitate of iron(III) hydroxide (Mr = 107) that is ….
a. 5.04 g d. 20.78 g
b. 10.70 g e. 25.75 g
c. 15.74 g
29. Calcium oxide reacts with phosphoric acid solution to form precipitate of calcium phosphate and water. That reaction as follow:
3CaO(s) + 2H3PO4(aq) Ca3(PO4)2(s) + 3H2O(l)
5 moles of phosphoric acid precisely reacts with alcium oxide. The moles amount of calcium oxide that reacts is ….
a. 0.5 mole d. 3 moles
b. 1 mole e. 7.5 molesl
c. 2 moles
30. 4 grams of the sample of impure sulfur is burnt to react with oxygen gas to produce 2.4 liters sulfur trioxide gas (RTP). (Ar O = 16, S = 32)
S(s) + O2(g) SO3(g) (not balanced)
The content of pure sulfur in the sample is ….
a. 40 % d. 90 %
b. 50 % e. 95 %
c. 80 %
31. The extraction of iron from its ore, Fe2O3, in the furnace occurs reaction as follow:
Fe2O3(s) + 3CO(g) 2Fe(s) + 3CO2(g)
In that extraction is produced 28 kg of the iron. The mass of iron ore, Fe2O3, that is extracted is …. (Ar C = 12, O = 16, Fe = 56)
a. 10 kg d. 40 kg
b. 16 kg e. 60 kg
c. 20 kg
32. 5.4 g of aluminum (Ar = 27) is reacted with 200 mL of 5 M hydrochloric acid solution to form aluminum chloride solution and hydrogen gas.
Al(s) + HCl(aq) AlCl3(aq) + H2(g) (not balanced)
The volume of hydrogen gas (RTP) that is produced in that reaction is ….
a. 2.40 L d. 9.60 L
b. 4.80 L e. 12.0 L
c. 7.20 L
33. The reaction between NH3 and O2 gas occurs as follow:
4NH3(g) + 5O2(g) 4NO(g) + 6H2O(l)
If in that reaction is reacted each of them is 0.5 moles, so NO gas that produced is…
a. 0.40 mole d. 2.00 moles
b. 0.75 mole e. 2.25 moles
c. 1.60 moles
34. A gaseous hydrocarbon compound has empirical formula of CH2. Known the mass of 5.6 L of the gaseous hydrocarbon compound (STP) is 14 g. The molecular formula of hydrocarbon compound is …
a. C2H4 d. C4H8
b. C2H6 e. C5H10
c. C3H6
35. An aqueous solution of electrolyte can transmit the electric current. The following is the best reason for this phenomenon. In the solution finds ….
a. the freely move ions
b. the freely move atoms.
c. the very active particles
d. the freely move molecules
e. the easily dissolve substances in the water
36. Among of the following solution groups, it which is classified as the strong electrolyte is …
a. acetic acid, hydrochloric acid, sodium hydroxide
b. hydrochloric acid, sodium hydroxide, potassium chloride
c. ammonia, sulfuric acid, sodium chloride
d. sodium hydroxide, sulfuric acid, ammonia
e. acetic acid, hydrochloric acid, ammonia
37. Pay attention to the following experiment pictures! .
Based on the fact that is shown by the picture above, so can be concluded that …
a. A solution is the strong electrolyte and B solution is non electrolyte
b. A solution is the non electrolyte and B solution is strong electrolyte
c. The number of ions in A solution is less than B solution
d. The number of ions in A solution is more than B solution
e. The number of ions in the solution can not be compared one another.
38. The following pair of compounds, it which is classified as the weak electrolyte is .…
a. C2H5OH, NH3(aq)
b. CH3COOH, NaCl
c. CO(NH2)2, C12H22O11
d. C6H12O6, NaOH
e. CH3COOH, NH3(aq)
39. Iron(III) nitrate in the aqueous solution undergoes ionization as follow::
Fe(NO3)3(aq) Fe3+(aq) + 3NO3−(aq)
Ionization degree (α) of Fe(NO3)3 = 1. If 0.5 mole of iron(III) nitrate is dissolved in the water until the solution volume of 500 mL, so the concentration of nitrate ions, NO3-, in the solution is ….
a. 1 M d. 4 M
b. 2 M e. 5 M
c. 3 M
40. 1.5 mole of ammonia is dissolved into the water so that to form the ammonia solution. In the solution, ammonia undergoes ionization according to the reaction equation:
NH3(aq) + H2O(l) NH+(aq) + OH− (aq)
In reality, in the solution exist 0.03 mole of OH- ion. Ionization degree (α) of ammonia is …
a. 0.01 d. 0.75
b. 0.02 e. 0.98
c. 0.25 (score 40)
II. Essays
Do the following problem
1. Given 17 grams of ammonia gas.
Determine the volume of ammonia gas that is measured at:
a. temperature of 27 0C , and pressure of 2 atm
b. the same condition of temperature and pressure (T.P), in which 2.5 liters of SO3 gas has mass of 8 grams.
(Ar N = 14, O = 16, S = 32) (score 6)
2. In analyze 4.5 g of carbon compound which consist of C, H. and O elements is found 0.1 g of hydrogen, 1.2 g of carbon and the remaining is oxygen.
Ar C = 12, H = 1, O = 16
a. Determine the empirical formula of carbon compound.
b. Known the relative molecular mass (Mr) of carbon compound is 90, determine the molecular formula of that carbon compound. (score 4)
3. Potassium phosphate solution and barium nitrate solution reacts to produce the precipitate of barium phosphate and potassium nitrate solution. In that reaction is reacted 150 mL of 0.2 M K3PO4 solution with 250 mL of 0.4 M Ba(NO3)2 solution.
a. Write the balanced reaction equation complete its physical state notation.
b. Calculate how many grams the mass of remaining reactant.
c. Calculate how many grams the mass of precipitate of Ba3(PO4)2. (Ar N = 14, O = 16, K = 39, P = 31, Ba = 137) (score 10)
4. 38 grams of solid hydrated sodium phosphate, Na3PO4.xH2O, is heated until all crystalline water to evaporate to produce 16.4 grams of solid anhydrous sodium phosphate, Na3PO4. Determine the chemical formula of that hydrated sodium phosphate.
(Ar H = 1 O = 16, Na = 23, P = 31) (score 6)
5. In the Iron(III) sulfate solution occurs ionization according to the equation as follow
Fe2(SO4)3(aq) Fe3+(aq) + SO42− (aq) not balanced)
Given 200 mL of solution that contains 4 moles of Fe2(SO4)3.
Ionization degree of Fe2(SO4)3 = 0.95.
a. Calculate the moles amount of Fe2(SO4)3 decomposes into ions
b. Calculate the concentration of Fe3+ ion in the solution in mole.L-1. (score 4)
