molecular formula chemistry homework help

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Chemistry library

Unit 1: atoms, compounds, and ions, unit 2: mass spectrometry, unit 3: chemical reactions and stoichiometry, unit 4: more about chemical reactions, unit 5: electronic structure of atoms, unit 6: periodic table, unit 7: chemical bonds, unit 8: gases and kinetic molecular theory, unit 9: states of matter and intermolecular forces, unit 10: chemical equilibrium, unit 11: acids and bases, unit 12: buffers, titrations, and solubility equilibria, unit 13: thermodynamics, unit 14: redox reactions and electrochemistry, unit 15: kinetics, unit 16: studying for the ap chemistry exam, unit 17: meet the chemistry professional.

(a) 12.01 amu; (b) 12.01 amu; (c) 144.12 amu; (d) 60.05 amu

(a) 123.896 amu; (b) 18.015 amu; (c) 164.086 amu; (d) 60.052 amu; (e) 342.297 amu

(a) 56.107 amu; (b) 54.091 amu; (c) 199.9976 amu; (d) 97.9950 amu

Use the molecular formula to find the molar mass; to obtain the number of moles, divide the mass of compound by the molar mass of the compound expressed in grams.

Formic acid. Its formula has twice as many oxygen atoms as the other two compounds (one each). Therefore, 0.60 mol of formic acid would be equivalent to 1.20 mol of a compound containing a single oxygen atom.

The two masses have the same numerical value, but the units are different: The molecular mass is the mass of 1 molecule while the molar mass is the mass of 6.022 × × 10 23 molecules.

(a) 256.528 g/mol; (b) 72.150 g mol −1 ; (c) 378.103 g mol −1 ; (d) 58.080 g mol −1 ; (e) 180.158 g mol −1

(a) 197.382 g mol −1 ; (b) 257.163 g mol −1 ; (c) 194.193 g mol −1 ; (d) 60.056 g mol −1 ; (e) 306.464 g mol −1

(a) 0.819 g; (b) 307 g; (c) 0.23 g; (d) 1.235 × × 10 6 g (1235 kg); (e) 765 g

(a) 99.41 g; (b) 2.27 g; (c) 3.5 g; (d) 222 kg; (e) 160.1 g

(a) 9.60 g; (b) 19.2 g; (c) 28.8 g

zirconium: 2.038 × × 10 23 atoms; 30.87 g; silicon: 2.038 × × 10 23 atoms; 9.504 g; oxygen: 8.151 × × 10 23 atoms; 21.66 g

AlPO 4 : 1.000 mol, or 26.98 g Al Al 2 Cl 6 : 1.994 mol, or 53.74 g Al Al 2 S 3 : 3.00 mol, or 80.94 g Al The Al2S3 sample thus contains the greatest mass of Al.

3.113 × × 10 25 C atoms

0.865 servings, or about 1 serving.

20.0 g H 2 O represents the least number of molecules since it has the least number of moles.

(a) % N = 82.24% % H = 17.76%; (b) % Na = 29.08% % S = 40.56% % O = 30.36%; (c) % Ca 2+ = 38.76%

% NH 3 = 38.2%

(a) CS 2 (b) CH 2 O

Mg 3 Si 2 H 3 O 8 (empirical formula), Mg 6 Si 4 H 6 O 16 (molecular formula)

C 15 H 15 N 3

We need to know the number of moles of sulfuric acid dissolved in the solution and the volume of the solution.

(a) 0.679 M ; (b) 1.00 M ; (c) 0.06998 M ; (d) 1.75 M ; (e) 0.070 M ; (f) 6.6 M

(a) determine the number of moles of glucose in 0.500 L of solution; determine the molar mass of glucose; determine the mass of glucose from the number of moles and its molar mass; (b) 27 g

(a) 37.0 mol H 2 SO 4 ; 3.63 × × 10 3 g H 2 SO 4 ; (b) 3.8 × × 10 −6 mol NaCN; 1.9 × × 10 −4 g NaCN; (c) 73.2 mol H 2 CO; 2.20 kg H 2 CO; (d) 5.9 × × 10 −7 mol FeSO 4 ; 8.9 × × 10 −5 g FeSO 4

(a) Determine the molar mass of KMnO 4 ; determine the number of moles of KMnO 4 in the solution; from the number of moles and the volume of solution, determine the molarity; (b) 1.15 × × 10 −3 M

(a) 5.04 × × 10 −3 M ; (b) 0.499 M ; (c) 9.92 M ; (d) 1.1 × × 10 −3 M

(a) 0.125 M ; (b) 0.04888 M ; (c) 0.206 M ; (e) 0.0056 M

(a) The dilution equation can be used, appropriately modified to accommodate mass-based concentration units: % mass 1 × mass 1 = % mass 2 × mass 2 % mass 1 × mass 1 = % mass 2 × mass 2 This equation can be rearranged to isolate mass 1 and the given quantities substituted into this equation. (b) 58.8 g

1.75 × × 10 −3 M

2.38 × × 10 −4 mol

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Molecular Formula

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• Gamini Gunawardena
• Utah Valley University

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The molecular formula of a covalent compound is the formula that shows the number of atoms of each element present in one molecule of the compound.

• eg. 1: The molecular formula of ethane is C 2 H 6 , meaning the ethane molecule contains two carbon atoms and six hydrogen atoms.
• eg. 2: The molecular formula of nicotine is C 10 H 14 N 2 , meaning the nicotine molecule contains ten carbon atoms, fourteen hydrogen atoms, and two nitrogen atoms.

see also structural formula , degree of unsaturation