Questions 27 to 30: Calculate the mass of each substance from the number of moles given. a) 0 .769 mol lithium chloride b) 57 .1 mol acetic acid, HC 2 H 3 O 2 c) 0 .68 mol lithium d) 0 .532 mol iron ( III ) sulfate e) 8 .26 mol sodium acetate (acetate ion, C 2 H 3 O 2 − )
Questions 27 to 30: Calculate the mass of each substance from the number of moles given. a) 0 .769 mol lithium chloride b) 57 .1 mol acetic acid, HC 2 H 3 O 2 c) 0 .68 mol lithium d) 0 .532 mol iron ( III ) sulfate e) 8 .26 mol sodium acetate (acetate ion, C 2 H 3 O 2 − )
Solution Summary: The author explains that the chemical formula for lithium chloride is LiCl. The number of moles is calculated using the formula given below.
[Tutorial: Empirical formula]
This question will walk you through the process of calculating the empirical
formula of a 100.0 g sample of an unknown compound from its elemental percent
compositions. This problem will be solved via the following sequence of
conversions: mass % mass moles mole ratio →
empirical formula.
Step 2: You have calculated that in a 100.0 gram sample of the unknown
compound, there are 4.76 moles of nitrogen, 2.38 moles of carbon, and 4.75
moles of hydrogen. Next, determine the simplest, whole-number ratio for each
element by dividing the number of moles of each by the smallest number of moles
(moles mole ratio). Which of the following represent the correct, normalized
mole ratio of the elements within the sample?
A) 4 C: 1H : 2 N
B) 1C:2 H: 2 N
moles
mole
ratio
mass
C) 1C:2 H: 1N
D) 2.38 C : 4.75 H: 4.76 N
E) 3 C:5 H:5 N
molecular struct..pdf
4. Convert 6.00 x 1021 atoms to mole of
sodium.
5. Convert 8.00 × 1023 molecules to mole of
water.
6. How many mole is 3.4 x 1026 formula
units of sodium chloride.
27) Determine the number of moles of compound within 25.0 g of Al(OH),
A) 0.321 mol
B) 36.03 mol
C) 0.594 mol
28) Determine the mass of the following compound: 0.0146 mol KOH
A) 56.11 g
B) 0.819 g
C) 8.19 g
29) Determine the mass of the following compound: 1.6 x 10-3 mol Na,sO,
A) 2.3 g
B) 0.23 g
C) 142.04 g
30) Diamond is one form of elemental carbon. An engagement ring contains a diamond weighing 1.25 carats (1
carat = 200 mg). How many atoms are present in the diamond?
A) 1.25 x 1022
B) 1.25 x 1020
C) 0.250
Chapter 7 Solutions
Introductory Chemistry: An Active Learning Approach
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Step by Step Stoichiometry Practice Problems | How to Pass ChemistryMole Conversions Made Easy: How to Convert Between Grams and Moles; Author: Ketzbook;https://www.youtube.com/watch?v=b2raanVWU6c;License: Standard YouTube License, CC-BY