what is the term for the value corresponding to the number of atoms in 12.01g of carbon?

(Last Updated On: March xviii, 2020)

This is the Multiples Option Questions Part 9 of the Series in General chemical science as one of the Full general Technology 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 diverse sources including past Board Questions in General Engineering science and Applied Sciences (GEAS) field.

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General Chemistry MCQs

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401. Decide the density of the infinite 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 10 x^-four k/cm3
• B. 3.71 10 x^-4 one thousand/cm3
• C. 7.31 x ten^-four g/cm3
• D. 8.31 ten 10^-4 g/cm3

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

• A. 3.85 moles
• B. 4.xv moles
• C. five.38 moles
• D. 3.35 moles

403. How many number of atoms are there in ane.32 x 10^3 g of Lead (Pb)? Lead atomic mass is 207.7g.

• A. three.84 x 10^23 atoms
• B. 4.38 x ten^23 atoms
• C. three.84 ten 10^24 atoms
• D. 4.38 10 10^24 atoms

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

• A. half dozen.95 ten 10^-3 grand
• B. five.45 x 10^-3 thousand
• C. 5.96 x 10^-iii thousand
• D. vii.59 x 10^-three grand

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

• A. 1.16 x x^-14 moles
• B. 1.61 ten 10^-thirteen moles
• C. one.sixteen ten x^-13 moles
• D. one.43 x x^-14 moles

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

• A. 3.51 10 x^3 chiliad
• B. iii.29 x x^three thousand
• C. 2.39 x 10^3 grand
• 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 cantlet
• B. one.21 x 10^-22 g/Ge atom
• C. 1.12 x 10^-22 m/Ge atom
• D. 1.31 x ten^-22 thou/Ge cantlet

408. Zinc (Zn) atom has atomic mass of 65.39. Calculate the number of atoms nowadays in four.22 g of zinc (Zn).

• A. 3.75 x 10^22 Zn atoms
• B. 3.93 x 10^22 Zn atoms
• C. 3.89 10 x^22 Zn atoms
• D. four.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 = one.008 g)

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

410. How many oxygen (O) atoms are at that place in 2.31 x x^4 chiliad of urea [(NH2)2CO]. Given molar mass of urea is sixty.062g.

• A. 2.43 x 10^26 atoms
• B. 2.12 x 10^26 atoms
• C. ii.32 ten 10^26 atoms
• D. 2.52 x 10^26 atoms

411. How many water molecules are present in 5.34 mL of h2o at a temperature of 4oC, which the density of water at this temperature is 1.00 1000/mL? Atomic masses of H and O are 1.008 chiliad and 16.00 yard respectively.

• A. ane.84 ten x^23 molecules
• B. 1.78 10 10^23 molecules
• C. i.74 10 10^23 molecules
• D. one.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 percentage limerick by mass: 19.8% C, 2.v% H, eleven.6% Due north. 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. Summate the molecular mass of methanol (CH4O), given the atomic masses of C = 12.01 g, H = 1.008 g and O = sixteen 1000.

• 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 chiliad of chloroform? C = 12.01 amu, H = i.008 amu and Cl = 35.45 amu.

• A. one.76 CHCl3 moles
• B. ii.12 CHCl3 moles
• C. iv.34 CHCl3 moles
• D. 2.51 CHCl3 moles

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

• A. 2.88 ten 1024 C atoms
• B. iii.72 x 1024 C atoms
• C. 2.54 x 1024 C atoms
• D. 2.00 x 1024 C atoms

416. What is the pct limerick by mass of oxygen (O) element in sulfuric acrid (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 sixteen.00 amu, respectively, how many grams of Al are in that location in 431g of Al2O3?

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

418. Which is the molecular formula of a sample of a compound containing half dozen.444 g of boron (B) and i.803 g of hydrogen (H)? The chemical compound has a molar mass of about 30 g. Given boron (B) has ten.81 amu and hydrogen (H) has one.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. Summate the molarity of a 90-mL ethanol (C2H5OH) solution which contains two.xv g of ethanol.

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

420. Decide the book in mL of stock solution that must be diluted to produce 3.00 x 10^ii mL of 0.856 M NaOH solution, starting with a five.27 G stock solution?

• A. 47.8 mL
• B. 48.vii 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 thou, calculate the per centum past 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. sixteen.75 50
• B. 13.84 L
• C. 15.76 L
• D. 16.48 Fifty

423. Summate the volume occupied by fifty.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 Fifty
• D. 1.38 L

424. Calculate the terminal force per unit area 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.eleven 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. one.99 ten 103 mm Hg
• B. 2.73 x 103 mm Hg
• C. ane.21 x 103 mm Hg
• D. two.13 10 103 mm Hg

426. Determine the last force per unit area of a gas, initially at 3.0 50, two.2 atm, and 72oC, which undergoes a change so that its concluding book and temperature are 0.9 50 and 41oC.

• A. 7.66 atm
• B. half dozen.67 atm
• C. four.18 atm
• D. v.73 atm

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

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

428. Calculate the molar mass of a certain gaseous organic compound having a density of 0.00356 g/mL at two.12 atm and 45oC.

• A. six.20 chiliad/mol
• B. 42.84 thou/mol
• C. 0.043 grand/mol
• D. four.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.v atm, and the mass of the gas was 0.0934g. B = 10.81 amu and H = one.008 amu.

• A. BH2
• B. BH3
• C. B2H6
• D. BH3

430. The atomic mass of chlorine is 35.45 k. What is the root-hateful-foursquare of molecular chlorine in yard/s at 31oC?

• A. 104 yard/south
• B. 10 m/due south
• C. 327 thousand/s
• D. 193 1000/s

431. Assuming there is no change in volume, decide the molarity of the acid solution if a three.12-L sample of hydrogen chloride gas at two.57 atm and 27.5oC, which is completely dissolved in a 700 mL of h2o to form hydrochloric acid solution.

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

432. A certain sample of natural gas contains 0.377 mole of ethane (C2H6), vii.48 moles of methane (CH4), and 0.134 mole of propane (C3H8). Calculate the partial force per unit area of propane gas, if the full pressure of the gases is ane.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 estrus of combustion of methanol, if the heat capacity of the flop plus water was eleven.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. lx.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 yard
• C. 177.32 thou
• D. 1.7732 yard

436. Calculate the number of molecules of oxygen gas present in 1.v L of air at STP. Assuming that air contains 31% O2, 67% N2 and 2% Ar, all by book.

• A. 1.87 x 10^23 molecules
• B. iv.18 10 ten^24 molecules
• C. 2.81 x x^23 molecules
• D. 1.25 x 10^22 molecules

437. Summate the mass of F in grams in 31.two 1000 of the compound Tin (Two) fluoride (SnF2), which is often added to toothpaste equally an ingredient for the prevention of tooth decay. Tin = 118.7 amu and Flourine = 19.00 amu.

• A. 3.78 g
• B. 7.57 1000
• C. 4.30 g
• D. 8.61 1000

438. Which of the following is the molar mass of the gas at 752 torr and 41oC? 10 grams of a gas occupy a book of 5.12 L.

• A. 51 thou/mol
• B. i.96 one thousand/mol
• C. 149 g/mol
• D. 1144 grand/mol

439. Make up one's mind the pressure exerted by hydrogen bromide (HBr) gas having a density of 2.978 thou/L at a temperature of 46oC. Hydrogen and bromine has diminutive 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 at that place in 7.xviii moles?

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

441. An instrument that separates particles of unlike 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 jump to the other components.

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

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

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

444. If a unmarried reactant is transformed past rut or electricity into ii 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. Barm flotation process

447. Which of the following does not change with modify 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 abiding composition
• C. The law of multiple proportions
• D. The law of chemical reaction

450. What kind of chemical bail will grade 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

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