Concept explainers
Compute the relative molecular masses of the following compounds on the
(a)
(c)
(e)
Want to see the full answer?
Check out a sample textbook solutionChapter 1 Solutions
EBK PRINCIPLES OF MODERN CHEMISTRY
- Give the name and formula of the compound formed from the following elements: (a) 12L and 9M (b) 30L and 16M (c) 17L and 38Marrow_forwardGive the name and formula of the compound formed from the following elements:(a) 12L and 9M (b) 30L and 16M (c) 17L and 38Marrow_forwardCapsaicin, the compound that gives the hot taste to chili peppers, has the formula C18H27NO3.(a) Calculate its molar mass.(b) If you eat 55 mg of capsaicin, what amount (moles) have you consumed?(c) Calculate the mass percent of each element in the compound.(d) What mass of carbon (in milligrams) is there in 55 mg of capsaicin?arrow_forward
- A compound has the composition of 54.53% Carbon, 9.15% Hydrogen, and 36.32% Oxygen, by mass. If the molar mass is 88.1 g/mol, what is its molecular formula? (A) C2H4O (B) C4H8O2 (C) C6H10O2 (D) C6H12O3arrow_forwardGive the number of atoms of the specified element in aformula unit of each of the following compounds, and calculatethe molecular (formula) mass:(a) Hydrogen in ammonium benzoate, C₆H₅COONH₄(b) Nitrogen in hydrazinium sulfate, N₂H₆SO₄(c) Oxygen in the mineral leadhillite, Pb₄SO₄(CO₃)₂(OH)₂arrow_forwardalculate (to the nearest 0.1 u) the formula mass of these compounds. (a) rubidium nitrate, RbNO3 u(b) carbon tetrachloride, CCl4 u(c) boron trifluoride, BF3 u Calculate (to the nearest 0.1 u) the formula mass of these compounds. (a) azithromycin, C38H72N2O12 u(b) saccharin, C7H5NO3S u(c) glucose, C6H12O6 uarrow_forward
- Capsaicin, the compound that gives the lhot taste to chili peppers, has the formula C18H27NO3.(a) Calculate its molar mass.(b) If you eat 55 mg of capsaicin, what amount (moles) have you consumed?(c) Calculate the mass percent of each element in the compound.(d) What mass of carbon (in milligrams) is there in 55 mg of capsaicin?arrow_forwardA compound Y containing carbon, hydrogen and oxygen only have the following composition by mass:C: 40.0% ; H: 6.7% ; O: 53.3%(a) Calculate the empirical formula of the compound. (Relative atomic masses: H =1.0, C = 12.0, O = 16.0) (b) Given that the relative molecular mass of compound Y is 180. Find its molecular formula.arrow_forwardGive the number of atoms of the specified element in a formula unit of each of the following compounds, and calculate the molecular (formula) mass:(a) Hydrogen in ammonium benzoate, C6H5COONH4(b) Nitrogen in hydrazinium sulfate, N2H6SO4(c) Oxygen in the mineral leadhillite, Pb4SO4(CO3)2(OH)2arrow_forward
- Calculate (to the nearest 0.1 u) the formula mass of these compounds. (a) acetaminophen, C8H9NO2 u(b) aspirin, C9H8O4 u(c) ibuprofen, C13H18O2 uarrow_forwardBefore the use of systematic names, many compounds had common names. Give the systematic name for each of the following: (a) Blue vitriol, CuSO4*5H2O (b) Slaked lime, Ca(OH)2 (c) Oil of vitriol, H2SO4 (d) Washing soda, Na2CO3 (e) Muriatic acid, HCl (f) Epsom salt, MgSO4*7H2O (g) Chalk, CaCO3 (h) Dry ice, CO2 (i) Baking soda, NaHCO3 (j) Lye, NaOHarrow_forward(a) In the certain hydrated salt MSO3⋅4H2O, the mass percentage of H2O is 44.71%. Identify the element M in the salt? (5 marks) (b) A certain element has two naturally occurring isotopes. (5 marks) The mass of one of the isotopes is 120.904 amu and its natural abundance is 57.21%. The mass of the second isotope is 122.904 amu. Calculate the average atomic mass Write the chemical symbols of the isotopesarrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning