If necessary, use the following data to answer the questions below.
Atomic Weight: H = 1.0, C = 12.0, N = 14.0, O = 16.0, S = 32.0, 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 noble gas?
(A) Ne
(B) Ar
(C) Br
(D) Kr
(E) Xe
QUESTION 02
Which of the following elements has the smallest electronegativity?
(A) K
(B) Cl
(C) Zn
(D) Li
(E) O
QUESTION 03
Which of the following atoms has the most valence electrons?
(A) N
(B) S
(C) Na
(D) Si
(E) F
QUESTION 04
Which of the following molecules has the most lone pair electrons?
(A) \(\ce{CH3OH}\)
(B) \(\ce{C2H4}\)
(C) \(\ce{NH3}\)
(D) \(\ce{CO2}\)
(E) \(\ce{HCl}\)
QUESTION 05
Which of the following oxides is an amphoteric oxide?
(A) \(\ce{NO2}\)
(B) \(\ce{CO2}\)
(C) \(\ce{Na2O}\)
(D) \(\ce{CaO}\)
(E) \(\ce{ZnO}\)
QUESTION 06
Which of the following compounds has the maximum mass percentage of carbon in the compound?
(A) \(\ce{CH3CHO}\)
(B) \(\ce{C2H5OH}\)
(C) \(\ce{CH3OCH3}\)
(D) \(\ce{CH3OH}\)
(E) \(\ce{CH3OH}\)
QUESTION 07
The volume percentage of hydrogen, \(\ce{H2}\), gas is 30% in a mixture of hydrogen gas and methane, \(\ce{CH4}\), gas at the standard state.
Answer the following questions.
(1) Calculate the density of the mixed gas.
(A) 0.28 g/L
(B) 0.53 g/L
(C) 2.8 g/L
(D) 5.3 g/L
(E) 28 g/L
(2) Calculate the heat evolved in a complete combustion of 10.0 L of the mixed gas at the standard state. The heats of combustion of hydrogen and methane are 286 and 891 kJ/mol, respectively.
(A) 103 kJ
(B) 209 kJ
(C) 317 kJ
(D) 421 kJ
(E) 533 kJ
QUESTION 08
The density of 17.0% sulfuric acid, \(\ce{H2SO4}\), is 1.12 g/mL. Calculate the molar concentration of the sulfuric acid.
(A) 0.9 mol/L
(B) 1.9 mol/L
(C) 2.9 mol/L
(D) 3.9 mol/L
(E) 4.9 mol/L
QUESTION 09
The solubilities of copper (II) sulfate, \(\ce{CuSO4}\), in water are 20 [g/100 g \(\ce{H2O}\)] at 293 K, and 54 [g/100 g \(\ce{H2O}\)] at 353 K. How many grams of copper (II) sulfate pentahydrate, \(\ce{CuSO4 5H2O}\), will crystallize out of 200 g of a solution saturated at 353 K if it cools to 293 K?
(A) 32 g
(B) 41 g
(C) 55 g
(D) 64 g
(E) 77 g
QUESTION 10
Calculate the degree of ionization, \(\alpha\), of \(1.0 \times 10^{-2} \text{ mol/L}\) acetic acid, \(\ce{CH3COOH}\). The ionization constant, Ka, of acetic acid is \(2.7 \times 10^{-5} \text{ mol/L}\). Use the following value, if necessary.
\(\sqrt{3} = 1.73\)
(A) 0.017
(B) 0.026
(C) 0.035
(D) 0.043
(E) 0.052
QUESTION 11
The mass of oxygen, \(\ce{O2}\), gas occupied a volume of 550 mL is 0.96 g at 330 K. Calculate the pressure of the oxygen gas.
QUESTION 12
In the following reaction, which of the following procedures is correct for the displacement of the equilibrium in the right direction?
\(\ce{N2 + 3 H2 <=> 2 NH3 + 92 kJ}\)
QUESTION 13
A certain amount of oxalic acid, \(\ce{(COOH)2}\), reacted with 200 mL of 0.020 mol/L potassium permanganate, \(\ce{KMnO4}\), to oxidize completely. Calculate the mass of the oxalic acid.
QUESTION 14
When electrolysis of a sulfuric acid, \(\ce{H2SO4}\), was carried out at 2.0 A for 25 min using a platinum, \(\ce{Pt}\), electrode, oxygen, \(\ce{O2}\), gas was liberated. Calculate the volume of the oxygen gas at the standard state.
QUESTION 15
Which of the following gases is the colored gas?
QUESTION 16
Which of the following metal complex ion solutions is the colored solution?
QUESTION 17
How many isomers are there for the compound with molecular formula \(\ce{C2H4O}\)?
QUESTION 18
Which of the following molecules has a positive reaction in the Fehling’s solution test?
QUESTION 19
Which of the following molecules does not react with ethylene \(\ce{CH2=CH2}\)?