MCQs in General Chemistry Part IX

(Last Updated On: December 8, 2017)

MCQs in General Chemistry Part 9

This is the Multiples Choice Questions Part 9 of the Series in General chemistry as one of the General Engineering and Applied Sciences (GEAS) topic. In Preparation for the ECE Board Exam make sure to expose yourself and familiarize in each and every questions compiled here taken from various sources including past Board Questions in General Engineering and Applied Sciences (GEAS) field.

Online Questions and Answers in General Chemistry Series

Following is the list of multiple choice questions in this brand new series:

General Chemistry MCQs
PART 1: MCQs from Number 1 – 50                        Answer key: PART I
PART 2: MCQs from Number 51 – 100                   Answer key: PART II
PART 3: MCQs from Number 101 – 150                 Answer key: PART III
PART 4: MCQs from Number 151 – 200                 Answer key: PART IV
PART 5: MCQs from Number 201 – 250                 Answer key: PART V
PART 6: MCQs from Number 251 – 300                 Answer key: PART VI
PART 7: MCQs from Number 301 – 350                 Answer key: PART VII
PART 8: MCQs from Number 351 – 400                 Answer key: PART VIII
PART 9: MCQs from Number 401 – 450                 Answer key: PART IX
PART 10: MCQs from Number 451 – 500                 Answer key: PART X

Continue Practice Exam Test Questions Part IX of the Series

Choose the letter of the best answer in each questions.

401. Determine the density of the space occupied by the electrons in the Na atom. The radius of the nucleus is given, and 3.04 fm. The radius of Na atom is 186 pm and atomic number is 11.

  • A. 4.21 x 10^-4 g/cm3
  • B. 3.71 x 10^-4 g/cm3
  • C. 7.31 x 10^-4 g/cm3
  • D. 8.31 x 10^-4 g/cm3

402. Calculate the moles of Magnesium (Mg) present in 93.5 g of Mg? (Mg atomic mass = 24.31g)

  • A. 3.85 moles
  • B. 4.15 moles
  • C. 5.38 moles
  • D. 3.35 moles

403. How many number of atoms are there in 1.32 x 10^3 g of Lead (Pb)? Pb atomic mass is 207.7g.

  • A. 3.84 x 10^23 atoms
  • B. 4.38 x 10^23 atoms
  • C. 3.84 x 10^24 atoms
  • D. 4.38 x 10^24 atoms

404. How many grams are there in 4.57 x 10^21 amu?

  • A. 6.95 x 10^-3 g
  • B. 5.45 x 10^-3 g
  • C. 5.96 x 10^-3 g
  • D. 7.59 x 10^-3 g

405. Calculate the number of moles of cobalt (Co) atom in seven billion Co atoms?

  • A. 1.16 x 10^-14 moles
  • B. 1.61 x 10^-13 moles
  • C. 1.16 x 10^-13 moles
  • D. 1.43 x 10^-14 moles

406. Given 16.7 moles of gold (Au), how many grams of Au are there? Atomic mass of Au is 197.0g.

  • A. 3.51 x 10^3 g
  • B. 3.29 x 10^3 g
  • C. 2.39 x 10^3 g
  • D. 3.76 x 10^3 g

407. Determine the mass in grams of a single atom of Ge which has an atomic mass of 72.59.

  • A. 2.21 x 10^-22 g/Ge atom
  • B. 1.21 x 10^-22 g/Ge atom
  • C. 1.12 x 10^-22 g/Ge atom
  • D. 1.31 x 10^-22 g/Ge atom

408. Zinc (Zn) atom has atomic mass of 65.39. Calculate the number of atoms present in 4.22 g of zinc (Zn).

  • A. 3.75 x 10^22 Zn atoms
  • B. 3.93 x 10^22 Zn atoms
  • C. 3.89 x 10^22 Zn atoms
  • D. 4.04 x 10^22 Zn atoms

409. Calculate for the number of molecules of ethane (C2H6) present in 0.431 g of C2H6. (C atomic mass = 12.01g; H atomic mass = 1.008 g)

  • A. 8.63 x 10^21 C2H6 molecules
  • B. 8.75 x 10^21 C2H6 molecules
  • C. 7.69 x 10^21 C2H6 molecules
  • D. 9.13 x 10^21 C2H6 molecules

410. How many oxygen (O) atoms are there in 2.31 x 10^4 g of urea [(NH2)2CO]. Given molar mass of urea is 60.062g.

  • A. 2.43 x 10^26 atoms
  • B. 2.12 x 10^26 atoms
  • C. 2.32 x 10^26 atoms
  • D. 2.52 x 10^26 atoms

411. How many water molecules are present in 5.34 mL of water at a temperature of 4oC, which the density of water at this temperature is 1.00 g/mL? Atomic masses of H and O are 1.008 g and 16.00 g respectively.

  • A. 1.84 x 10^23 molecules
  • B. 1.78 x 10^23 molecules
  • C. 1.74 x 10^23 molecules
  • D. 1.87 x 10^23 molecules

412. Which of the following is the molecular formula of peroxyacylnitrate (PAN), one of the components of smog, and is a compound of C, H, N, O, with percent composition by mass: 19.8% C, 2.5% H, 11.6% N. Given that its molar mass is about 120 g. ( Atomic masses: C = 12.01g; H = 1.008g; N = 14.01g; O = 16.00g).

  • A. C2H3NO2
  • B. C2H5NO3
  • C. C4H6N2O10
  • D. C2H3NO5

413. Calculate the molecular mass of methanol (CH4O), given the atomic masses of C = 12.01 g, H = 1.008 g and O = 16 g.

  • A. 29.018 amu
  • B. 34.241 amu
  • C. 32.042 amu
  • D. 30.026 amu

414. How many moles of chloroform (CHCl3) are there in 210.45 g of chloroform? C = 12.01 amu, H = 1.008 amu and Cl = 35.45 amu.

  • A. 1.76 CHCl3 moles
  • B. 2.12 CHCl3 moles
  • C. 4.34 CHCl3 moles
  • D. 2.51 CHCl3 moles

415. The atomic masses of carbon, hydrogen, and oxygen are 12.07g, 1.008g and 16.00g respectively. Calculate the number of C atoms present in 84.5 g of isopropanol (rubbing alcohol), C3H8O?

  • A. 2.88 x 1024 C atoms
  • B. 3.72 x 1024 C atoms
  • C. 2.54 x 1024 C atoms
  • D. 2.00 x 1024 C atoms

416. What is the percent composition by mass of oxygen (O) element in sulfuric acid (H2SO4)? H = 1.008 amu, S = 32.07 amu, S = 32.07 amu and O = 16.00 amu.

  • A. 62.25 %
  • B. 63.34 %
  • C. 64.45 %
  • D. 65.25 %

417. If atomic masses of Al and O are 26.98 amu and 16.00 amu, respectively, how many grams of Al are there in 431g of Al2O3?

  • A. 228 g
  • B. 215 g
  • C. 237 g
  • D. 114 g

418. Which is the molecular formula of a sample of a compound containing 6.444 g of boron (B) and 1.803 g of hydrogen (H)? The compound has a molar mass of about 30 g. Given boron (B) has 10.81 amu and hydrogen (H) has 1.008 amu.

  • A. B2H3
  • B. BH
  • C. B2H6
  • D. BH3

419. The atomic masses of carbon, hydrogen, and oxygen are 12.01g, 1.008g, and 16g respectively. Calculate the molarity of a 90-mL ethanol (C2H5OH) solution which contains 2.15 g of ethanol.

  • A. 0.52 M
  • B. 0.25 M
  • C. 0.61 M
  • D. 0.44 M

420. Determine the volume in mL of stock solution that must be diluted to produce 3.00 x 10^2 mL of 0.856 M NaOH solution, starting with a 5.27 M stock solution?

  • A. 47.8 mL
  • B. 48.7 mL
  • C. 51.2 mL
  • D. 48.1 mL

421. Bromine (Br) and Silver has atomic masses of 79.90g and 107.9g, respectively. In a certain experiment, a sample of 0.3320g of an ionic compound containing the bromide ion (BrI) is dissolved in water and treated with an excess of AgNO3 if the mass of the AgBr precipitate that forms is 0.734 g, calculate the percent by mass of Br in the original compound?

  • A. 42.55 %
  • B. 49.70 %
  • C. 84.10 %
  • D. 94.07 %

422. Solve for the volume occupied by 3.12 moles of nitric oxide (NO) which exerts 5.43 atm of pressure at a temperature of 82oC.

  • A. 16.75 L
  • B. 13.84 L
  • C. 15.76 L
  • D. 16.48 L

423. Calculate the volume occupied by 50.6 g of HCl at STP. H = 1.008 amu and Cl = 35.45 amu.

  • A. 83.2 L
  • B. 31.1 L
  • C. 27.4 L
  • D. 1.38 L

424. Calculate the final pressure if a sample of a certain gas is cooled from 34oC to -73oC, with an initial pressure of 1.45 atm.

  • A. 1.42 atm
  • B. 3.11 atm
  • C. 0.94 atm
  • D. 1.63 atm

425. An 867-mL sample of chlorine gas exerts a pressure of 738 mmHg. Determine the pressure of the gas if the volume is reduced to 321 mL at constant temperature.

  • A. 1.99 x 103 mm Hg
  • B. 2.73 x 103 mm Hg
  • C. 1.21 x 103 mm Hg
  • D. 2.13 x 103 mm Hg

426. Determine the final pressure of a gas, initially at 3.0 L, 2.2 atm, and 72oC, which undergoes a change so that its final volume and temperature are 0.9 L and 41oC.

  • A. 7.66 atm
  • B. 6.67 atm
  • C. 4.18 atm
  • D. 5.73 atm

427. Calculate the density of uranium hexafluoride (UF6) with pressure of 697 mmHg at 57oC temperature. Atomic masses: U = 238 g; F = 19 g.

  • A. 90.55 g/L
  • B. 52.42 g/L
  • C. 68.98 g/L
  • D. 11.92 g/L

428. Calculate the molar mass of a certain gaseous organic compound having a density of 0.00356 g/mL at 2.12 atm and 45oC.

  • A. 6.20 g/mol
  • B. 42.84 g/mol
  • C. 0.043 g/mol
  • D. 4.384 g/mol

429. Determine the molecular formula of a gaseous compound which is 78.14% boron and 21.86% H. At a temperature of 27oC, 33.2864-mL of the gas exerted a pressure of 2.5 atm, and the mass of the gas was 0.0934g. B = 10.81 amu and H = 1.008 amu.

  • A. BH2
  • B. BH3
  • C. B2H6
  • D. BH3

430. The atomic mass of chlorine is 35.45 g. What is the root-mean-square of molecular chlorine in m/s at 31oC?

  • A. 104 m/s
  • B. 10 m/s
  • C. 327 m/s
  • D. 193 m/s

431. Assuming there is no change in volume, determine the molarity of the acid solution if a 3.12-L sample of hydrogen chloride gas at 2.57 atm and 27.5oC, which is completely dissolved in a 700 mL of water to form hydrochloric acid solution.

  • A. 0.644 M
  • B. 0.000464 M
  • C. 0.464 M
  • D. 0.0464 M

432. A certain sample of natural gas contains 0.377 mole of ethane (C2H6), 7.48 moles of methane (CH4), and 0.134 mole of propane (C3H8). Calculate the partial pressure of propane gas, if the total pressure of the gases is 1.79 atm.

  • A. 1.68 atm
  • B. 0.084 atm
  • C. 0.94 atm
  • D. 0.03 atm

433. A 2.102g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently, the temperature of the water was rose by 5.13oC. Solve for the molar heat of combustion of methanol, if the heat capacity of the bomb plus water was 11.8 kJ/oC. Carbon has 12.01 amu, hydrogen has 1.008 amu and oxygen has 16.00 amu.

  • A. 922.75 kJ/mol
  • B. – 922.75 kJ/mol
  • C. 60.534 kJ/mol
  • D. – 28.79 kJ/mol

434. Caffeine (C8H10N4O2) is a stimulant found in tea and coffee. What is its empirical formula?

  • A. C4H5N2O
  • B. C5H3NO2
  • C. C2H6NO3
  • D. C8H10N4O2

435. Calculate the mass of a piece of platinum metal with a density of 34.1 g/cm3 and has a volume of 5.2 cm3.

  • A. 17.732 g
  • B. 1773.2 g
  • C. 177.32 g
  • D. 1.7732 g

436. Calculate the number of molecules of oxygen gas present in 1.5 L of air at STP. Assuming that air contains 31% O2, 67% N2 and 2% Ar, all by volume.

  • A. 1.87 x 10^23 molecules
  • B. 4.18 x 10^24 molecules
  • C. 2.81 x 10^23 molecules
  • D. 1.25 x 10^22 molecules

437. Calculate the mass of F in grams in 31.2 g of the compound Tin (II) fluoride (SnF2), which is often added to toothpaste as an ingredient for the prevention of tooth decay. Tin = 118.7 amu and Flourine = 19.00 amu.

  • A. 3.78 g
  • B. 7.57 g
  • C. 4.30 g
  • D. 8.61 g

438. Which of the following is the molar mass of the gas at 752 torr and 41oC? Ten grams of a gas occupy a volume of 5.12 L.

  • A. 51 g/mol
  • B. 1.96 g/mol
  • C. 149 g/mol
  • D. 1144 g/mol

439. Determine the pressure exerted by hydrogen bromide (HBr) gas having a density of 2.978 g/L at a temperature of 46oC. Hydrogen and bromine has atomic masses of 1.008g and 79.9 g, respectively.

  • A. 73 mm Hg
  • B. 106 mm Hg
  • C. 733 mm Hg
  • D. 0.964 mm Hg

440. How many grams of mercury (Hg = 200.6 amu) are there in 7.18 moles?

  • A. 0.036 g
  • B. 1440 g
  • C. 312 g
  • D. 1004 g

441. An instrument that separates particles of different isotopic composition and measure their individual relative masses.

  • A. mass spectrometer
  • B. barometer
  • C. hygrometer
  • D. hydrometer

442. These are compounds containing water molecules loosely bound to the other components.

  • A. isotope
  • B. hydrates
  • C. ion
  • D. mixture

443. If a more active element replaces a less active one in a compound, the reaction is:

  • A. combustion reactions
  • B. replacement reactions
  • C. metathesis
  • D. neutralization

444. If a single reactant is transformed by heat or electricity into two or more products, the type of reaction is

  • A. decomposition
  • B. combination
  • C. displacement
  • D. double displacement

445. The numerical value for standard pressure of any gas is

  • A. 76 mm Hg
  • B. 760 cm Hg
  • C. 760 mm Hg
  • D. 7.6 cm Hg

446. Any process extracting the metal in a fused state is called

  • A. Calcination
  • B. Roasting
  • C. Smelting
  • D. Froth flotation process

447. Which of the following does not change with change in temperature?

  • A. volume
  • B. mass
  • C. pressure
  • D. density

448. A device used to measure density.

  • A. manometer
  • B. hydrometer
  • C. spectrometer
  • D. densimeter

449. The statement “mass is neither created nor destroyed in a chemical reaction” is known as:

  • A. The law of conservation of mass
  • B. The law of constant composition
  • C. The law of multiple proportions
  • D. The law of chemical reaction

450. What kind of chemical bond will form in binary compounds where the electronegativity difference between atoms is greater than 2.0

  • A. Ionic Bond
  • B. Covalent Bond
  • C. Metallic Bond
  • D. Chemical Bond

Complete List of MCQs in General Engineering and Applied Science per topic

MCQs in General Chemistry Part IX
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