7. Calculate the molar mass of each of the following compounds. a. Fe,O,, iron(III) oxide b. BCl, boron trichloride c. CoHgO6, ascorbic acid (vitamin C) 8. Calculate the molar masses (in grams per mole) of each of the following. a. cane sugar, C12H2½0¡1 b. laughing gas, N¿O c. vitamin A, C20H300 9. Calculate the molar mass of each these compounds and the mass percentage of each element. a. PbS, lead(II) sulfide, galena b. C,H6, ethane, a hydrocarbon fuel c. CH;COOH, acetic acid, an important ingredient in vinegar d. NH¼NO3, ammonium nitrate, a fertilizer

7. Calculate the molar mass of each of the following compounds. a. Fe,O,, iron(III) oxide b. BCl, boron trichloride c. CoHgO6, ascorbic acid (vitamin C) 8. Calculate the molar masses (in grams per mole) of each of the following. a. cane sugar, C12H2½0¡1 b. laughing gas, N¿O c. vitamin A, C20H300 9. Calculate the molar mass of each these compounds and the mass percentage of each element. a. PbS, lead(II) sulfide, galena b. C,H6, ethane, a hydrocarbon fuel c. CH;COOH, acetic acid, an important ingredient in vinegar d. NH¼NO3, ammonium nitrate, a fertilizer

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

What is the mass (g) of 0.826 moles of acetic acid? The molar mass of HC2H3O2 is 60.06 g/mol. a. 72.7 b. 49.6 c. 51.8 d. 0.0138
3. The average atomic mass of an atom is expressed in c. g/mol a. grams 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 16g of CH4 d. 4 moles of CH4 is equal to 64 g of CH4
17. What is the molecular formula if the empirical formula is C2HS and the molecular molar mass is 58.14 g/mol? A. CH2.5 O B. CZHS C. CAH8 O D. C4H10 18. A compound with molecular mass of 74.1 g/mol is found to contain 64.8% carbon, 13.5% hydrogen, and 21.7% oxygen. What is the molecular formula? O A. CH20 B. C2H602 C. C4H100 D. C4H1003
a. A compound is 54.53% C, 9.15% H, and 36.32% O by mass. What is its empirical formula? b. The molecular mass of a compound is 132 amu. What is its molecular formula?
Ibuprofen is an anti-inflammatory with the formula C13H18O2 A. What is the molar mass of ibuprofen? Express your answer using four significant figures. B. How many grams of ibuprofen are in 0.505 mole? Express your answer using three significant figures. C. How many moles of carbon are in 12.5 g of ibuprofen? Express your answer using three significant figures. D. How many moles of ibuprofen contain 1.42×1023 atoms of carbon? Express your answer using three significant figures. please solve all stepwise
Which substance has the largest molar mass A. Water B. Carbon dioxide C. Methane (CH_4) D. Iodine (I_2) E. Hydrogen chloride (HCI)
he Tragedy of Ha... O 24 mol O 2.0 mol Carbon dioxide can be produced by burning carbon in oxygen: C + O₂ → CO₂ Approximately how many moles of carbon dioxide can be created from 24.0 g C? O 12 mol 22 mol O 44 mol O 0.20 mol O 0.50 mol 4.01 Content - Che... Q Search PRO CON Should Pit Bulls Be... CELO
A compound is found to contain 7.522% phosphorus and 92.47 % iodine by mass. a. What is the empirical formula for the compound? b. The molar mass for this compound is 411.7 g/mol. What is the molecular formula?
2. The chemical formula for the active ingredient in the anti-inflammatory drug Celebrex is C17H14F3N3O2S. a. What is the molar mass of C17H14F3N3O2S? b. How many moles are in 10.0 g of C17H14F3N3O2S? C. How many molecules are in 10.0 g of C17H14F3N3O2S?
a. Calculate the number of moles in 21.7 mg of nitrogen dioxide. mol b. Calculate the number of moles in 1.70 g of copper(II) nitrate. mol c. Calculate the number of moles in 2.46 g of carbon disulfide. mol
C. Calculate the number of atoms or molecules in each of the following samples. 19) 0.357 moles of potassium 20) 2.93 moles of Ca 21) 473 moles of CuSO4 22) An 85.5-g sample of Hg in a barometer 23) A 0.251-g Ti metal heart valve 24) A 10.0-g sample of N₂0 gas
Consider 68.9 g of Pb(SO4)2 to answer the following questions. a. How many moles of Pb(SO4)2 is this? ____________________________ b. How many molecules of Pb(SO4)2 is this? ____________________________ c. What is the weight of one molecule of Pb(SO4)2 in amu? _________________ d. How many grams are 4.23 x 1022 molecules? __________________________