If necessary, use the following data to answer the questions below.
Atomic Weight: H = 1.0, C = 12.0, O = 16.0, Na = 23.0, Cl = 35.5, Cu = 64.0
Molar volume of gas at the standard state: 22.4 L/mol
Gas constant: = 0.082 atm L / (Kmol) = 8.31 × 103 Pa L/(Kmol)
Avogadro constant: A = 6.02 × 1023 /mol
Pressure: 1 atm = 1.01 × 105 Pa = 760 mmHg
Faraday constant: = 9.65 × 104 C / mol
Choose the correct answer from the choices to below. Select the closest one, when your calculated result does not exactly match any of the values of the alternatives in each group.
QUESTION 01
Which of the following elements is not the typical element?
(A) Zn
(B) Mn
(C) Ca
(D) Si
(E) Ar
QUESTION 02
Which of the following atoms has a different number of neutrons from electrons?
(A) \(\ce{^4He}\)
(B) \(\ce{^{14}N}\)
(C) \(\ce{^{16}O}\)
(D) \(\ce{^{32}S}\)
(E) \(\ce{^{39}K}\)
QUESTION 03
Which of the following atoms has the smallest number of valence electrons?
(A) Cl
(B) Be
(C) aAl
(D) Ne
(E) Na
QUESTION 04
Which of the following molecules has the same number of shared electron pairs as unshared electron pairs in one molecule?
(A) \(\ce{CO2}\)
(B) \(\ce{N2}\)
(C) \(\ce{O2}\)
(D) \(\ce{C2H4}\)
(E) \(\ce{NH3}\)
QUESTION 05
Which of the following salts show acidic when it dissolves in water?
(A) \(\ce{Na2CO3}\)
(B) \(\ce{CaCl2}\)
(C) \(\ce{NH4Cl}\)
(D) \(\ce{CH3COONa}\)
(E) \(\ce{K2SO4}\)
QUESTION 06
A 250 mL solution is produced by dissolving 0.10 g of sodium hydroxide in sufficient water. What is the pH of this solution?
(A) 1
(B) 2
(C) 11
(D) 12
(E) 13
QUESTION 07
When 10 mL of 1.0 mol/L sulfuric acid reacts with 1.0 g of \(\ce{NaOH}\), how much reactant will be left after the reaction is completed?
(A) 0.74 g \(\ce{H2SO4}\)
(B) none of either compound
(C) 0.20 g \(\ce{NaOH}\)
(D) 0.40 g \(\ce{NaOH}\)
(E) 0.60 g \(\ce{NaOH}\)
QUESTION 08
Calculate the density [g/L] of hydrogen, \(\ce{H2}\), gas at standard state.
(A) 0.045 g/L
(B) 0.089 g/L
(C) 0.18 g/L
(D) 0.45 g/L
(E) 0.89 g/L
QUESTION 09
The solubilities of potassium nitrate, \(\ce{KNO3}\), in water are 40 [g/100 g \(\ce{H2O}\)] at 27°C, and 169 [g/100 g \(\ce{H2O}\)] at 80°C. How many grams of potassium nitrate will crystallize out, when 100 g of the saturated potassium nitrate solution at 80°C is cooled to 27°C?
(A) 12 g
(B) 24 g
(C) 48 g
(D) 60 g
(E) 69 g
QUESTION 10
How much heat is released by the following reaction when 0.25 mol of sodium reacts completely with chlorine?
\(\ce{2 Na (s) + Cl2 (g) -> 2 NaCl (s) + 822 kJ}\)
(A) 103 kJ
(B) 206 kJ
(C) 411 kJ
(D) 822 kJ
(E) 1644 kJ
QUESTION 11
In the following reaction, which has the increased oxidation number of the underlined element by the reaction?
(A) \(2 \underline{\ce{H}} \ce{_2O + 2 K -> 2 KOH + } \underline{\ce{H}}_2\)
(B) \(\underline{\ce{Cl}} \ce{_2 + 2 KBr -> 2 K} \underline{\ce{Cl}} \ce{+ Br2}\)
(C) \(\underline{\ce{S}} \ce{O2 + 2 H2S -> 3 \underline{\ce{S}} + 2 H2O}\)
(D) \(\ce{H2} \underline{\ce{O}}\ce{_2} \ce{ + SO2 -> H2S} \underline{\ce{O}} \ce{_4}\)
(E) \(\underline{\ce{S}} \ce{O2 + Br2 + 2H2O -> H2} \underline{\ce{S}} \ce{O4 + 2HBr}\)
QUESTION 12
9.5 mL of 0.20 mol/L potassium permanganate, \(\ce{KMnO4}\), aqueous solution was required to oxidize 20 mL of tin (II) chloride, \(\ce{SnCl2}\), solution with unknown concentration in sulfuric acid. Calculate the molar concentration of the tin (II) chloride aqueous solution. However, at this time, it is assumed that only the following reactions have occurred.
\(\ce{MnO4- + 8H+ + 5e- -> Mn^{2+} + 4H2O}\)
\(\ce{Sn^{2+} -> Sn^{4+} + 2e-}\)
(A) 0.038 mol/L
(B) 0.095 mol/L
(C) 0.19 mol/L
(D) 0.24 mol/L
(E) 0.48 mol/L
QUESTION 13
A copper (II) chloride, \(\ce{CuC2}\), aqueous solution was electrolyzed at a current of 1.93 A for 8 minutes and 20 seconds using a carbon, \(\ce{C}\), electrode. Calculate the mass of the substance produced at the cathode.
(A) 0.160 g
(B) 0.320 g
(C) 0.640 g
(D) 1.28 g
(E) 3.20 g
QUESTION 14
When 1.15 g of a volatile liquid was completely evaporated at 127°C, the liquid turned into 831 mL of vapor at 1.0 × 105 Pa. Calculate the molecular weight of this liquid substance.
(A) 15
(B) 20
(C) 32
(D) 46
(E) 83
QUESTION 15
When a closed flask of constant capacity holds 2.0 mol each of hydrogen and iodide at a temperature of 30°C, 3.2 mol of hydrogen iodide is produced at equilibrium. Calculate the equilibrium constant K of this reaction.
(A) 1.6
(B) 2.6
(C) 8.0
(D) 20
(E) 64
QUESTION 16
If 68.4 g of sucrose (molecular weight = 342) is dissolved in 500 g of water, what will be the freezing point of this solution? The molar freezing point descent of water is 1.85 K·kg/ mol.
(A) \(-7.40 \times 10^{-4} \: ^{\text{o}} \text{C}\)
(B) \(-3.70 \times 10^{-2} \: ^{\text{o}} \text{C}\)
(C) \(-1.85 \times 10^{-1} \: ^{\text{o}} \text{C}\)
(D) \(-3.70 \times 10^{-1} \: ^{\text{o}} \text{C}\)
(E) \(-7.40 \times 10^{-1} \: ^{\text{o}} \text{C}\)
QUESTION 17
How many isomers are there for the compound with molecular formula \(\ce{C3H8O}\)?
(A) 1
(B) 2
(C) 3
(D) 4
(E) 5
QUESTION 18
Which of the following compounds show a silver mirror reaction?
(A) \(\ce{HCOOH}\)
(B) \(\ce{CH3COOH}\)
(C) \(\ce{CH3OH}\)
(D) \(\ce{CH3COCH3}\)
(E) \(\ce{CH2=CH2}\)
QUESTION 19
Which of the following compounds is produced when a mixture of ethanol and concentrated sulfuric acid are heated to about 170°C ?
(A) \(\ce{CH2=CH2}\)
(B) \(\ce{CH3CHO}\)
(C) \(\ce{HCOOH}\)
(D) \(\ce{CH3OCH3}\)
(E) \(\ce{C2H5OC2H5}\)
QUESTION 20
An unknown compound has the following percentage composition by weight: C = 54.5%, H = 9.1% and O = 36.4%. Its molecular weight is 88. Which is the molecular formula of this compound?
(A) \(\ce{CH2O}\)
(B) \(\ce{C2H4O}\)
(C) \(\ce{C3H4O3}\)
(D) \(\ce{C4H8O2}\)
(E) \(\ce{C5H12O}\)