5. Aspartame is an artificial sweetener that is 160 times sweeter than sucrose (table sugar) when dissolved in water. It is marketed as Nutra-Sweet. The molecular formula of aspartame is C14H18N2O5. Calculate the following d. What number of molecules are in 5.0 mg aspartame e. What number of atoms of nitrogen are in 1.2 g aspartame f. What is the mass in grams of 1.0 x 109 molecules of aspartame

5. Aspartame is an artificial sweetener that is 160 times sweeter than sucrose (table sugar) when dissolved in water. It is marketed as Nutra-Sweet. The molecular formula of aspartame is C14H18N2O5. Calculate the following d. What number of molecules are in 5.0 mg aspartame e. What number of atoms of nitrogen are in 1.2 g aspartame f. What is the mass in grams of 1.0 x 109 molecules of aspartame

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Mixtures are divided into two classes based 1. mixtures and matter on their appearance. classes? What are these two O 2. compounds and solutions O 3. homogeneous and mixtures O 4. elements and compounds O 5. homogeneous and heterogeneous
4. A hydrocarbon has the following centesimal composition: 17.24% hydrogen and 82.74% carbon. The molecular mass of the compound is 58g/mol. The atomic masses: H=1; C=12.What are the empirical and true formulas of this compound? A) CH yC2H5 B) C2H5 and C8H16 C) C2H5 and C4H10 D) C4H10 C8H20 E) None of the above
For quick access, place your favorites here on the favorites bar. Manage favorites now 66°F Mostly cloudy What quantity in moles of silver atoms do you have if you have 5.08 × 1021 atoms of silver. (The mass of one mole of silver is 107.87 g.) H Question 1 of 21 Ơ 837 $0
5. Knowing that one mole of water has a mass of 18,02 grams, calculate the number of molecules in ONE drop of water. (1 mL H2O = 20 drops H2O, Density of H2O = 1.00 g/mL) i mol of H20 = 18.029 %3D 6. If this drop of water was stretched so that the individual molecules would line up end-to-end, how long (in miles) would that line be? (1 molecule of H2O = 2 x 10-10 m, 1 km 6.2 x 10- mile) ompound with the formula MI4. The compound contains 71.00% I by mass. Identify
H. H. Three moles of the compound in the figure above would weigh how many grams? (The atomic masses, in daltons, are approximately 12 for carbon, 1 for hydrogen). O=U エーO CH
a. How many ATOMS of sulfur are present in 4.49 grams of sulfur tetrafluoride? ues if needed for this question. atoms of sulfur. b. How many GRAMS of fluorine are present in 1.07 × 1023 molecules of sulfur tetrafluoride? grams of fluorine.
The chemical Oswegium pantherides formula is Os3Pa2. Oswegium’s (Symbol Os) atomic mass is 10 grams and pantheride ‘s (Symbol Pa) atomic mass is 5 grams. Calculate the percent composition of Oswegium in Oswegium pantheride ( Os3Pa2).
29
II. Determine the empirical formula formulas of the following compounds given their molecular formulas.
9. How many hydrogen atoms are there in 500.0 L of water? (dH₂O = 1.00 g mL¯¹) A: 3.34 x 1028
2. g/mL. Determine the number of hydrogen atoms in one liter of water. The density of water is 1