Calculate each of the following:
a. number of C atoms in 0.500 mol of C
b. number of
c. moles of Fe in
d. moles of
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Basic Chemistry
- 40. Calculate the number of moles in each of the followine of NaCl a. 32.3 grams b. 11.6 grams of CO2 c. 508.3 grams of C,H, 42. Calculate the number of moles in each of the following: a. 123.5 g of KCIO b. 17.3 g of H, c. 11.6 mg of Ca(CIO,)2 44. Convert each of the following to moles and to atoms: a. 18.7 grams of calcium metal b. 51.9 grams of tellurium, Te c. 178.4 grams of uranium, Uarrow_forwardHow many moles of Ca3(PO4)2 are in 1.00 g of Ca3(PO4)2? (Use whole molar masses from periodic table and choose closest calculated answer) a.6.022 x 1023 moles b.310. moles c.3.10 x 10-3 moles d.1.00 mole e.3.22 x 10 3 moles e byarrow_forward1211 2. 1ouprofen, the anit-inflammatory ingredient in Advil, has the formula C13HIBO2. a. How many molecules are in 0.200 mole ibuprofen? b. How many H atoms are in 0.100 mole ibuprofen? c. How many moles of ibuprofen contain 7.4x10²5 atoms of C? d. What is the molar mass of ibuprofen?arrow_forward
- How many moles of carbon are in 7.50 g of the compound C3H4O2? Atomic Mass: C = 12.01; H = 1.008; O =16.00 g/mole Select one: of O a. 0.104 mole O b. 0.416 mole tion O c. 0.208 mole O d. 0.312 mole Next page 7:03 PM 4/7/2021arrow_forward2. Calculate the number of moles and grams from the following: (use correct sig figs in answer) a. 3.510 x 1022 molecules of PCl5 b. 4.386 x 1023 molecules of MgSO43. a. Find the empirical formula of a compound containing 36.89 %C, 13.96 %H, and 49.15 %O. b. Find the molecular formula for the compound with a molar mass of 260.44g/mole.4. Calculate the mass percent of each element in the following chemical formula: C4H11O3N2arrow_forwardIbuprofen, the anit-inflammatory ingredient in Advil, has the formula C13H18O2. a. How many molecules are in 0.200 mole ibuprofen? b. How many H atoms are in 0.100 mole ibuprofen? c. How many moles of ibuprofen contain 7.4x1025 atoms of C?arrow_forward
- a. How many moles of tetraphosphorus decaoxide, P4010, are present in a sample that contains 7.35 moles of oxygen atoms? mol P4O10 b. How many moles of oxygen atoms are present in a sample that contains 3.03 moles of P4010? mol Oarrow_forwardA single molecule of a certain compound has a mass of 3.4 x10-22g. Which value comes closet to the mass mass of a mole of thi compoumd? Choice A 50 g.mol-1 B 100 g.mol-1 C 150 g.mol-1 D180 g.mol-1arrow_forwardA 1.375 g sample of mannitol, a sugar found in seaweed, is burned completely in oxygen to give 1.993 g of carbon dioxide and 0.9519 g of water. The empirical formula of mannitol is Select one: a. CHO b. C3H7O3 c. CH2O d. CH7O3 e. C3H2Oarrow_forward
- 3. The average atomic mass of an atom is expressed in a. grams c. g/mol b. amu d. moles 4. Which statement is correct? a. 4 g of CH4 is equal to 4 moles of CH4 b. 4 g of CH4 is equal to 1 mole of CH4 C. 4 moles of CH4 is equal to 16 g of CH4 d. 4 moles of CH4 is equal to 64 g of CH4 5. Which statement is NOT true? a. One mole of a substance contains a fixed number of particles. b. One mole each of different substances have different masses and different number of particles. c. One mole each of different substances have the same number of particles but they have different masses. d. The formula mass of the compound is equal to one mole of that substance.arrow_forwardWhat is the empirical formula for the given MF:C5HI12 O a. C5H12 O b. CH O c. CH6arrow_forwardFind the empirical formula for a compound with the mass percent composition of 68.42 % Chromium and 31.58 % Oxygen. Select one: a. none of these b. CrO3 c. CrO2 d. Cr2O5 e. CrO f. Cr2O g. Cr2O3arrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781285199023Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning