Concept explainers
How many chlorine atoms are in each of the following?
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Chapter 4 Solutions
Chemistry In Focus
- Natural rubidium has the average mass of 85.4678 u and is composed of isotopes 85Rb (mass = 84.9117 u) and 87Rb. The ratio of atoms 85Rb/ 87Rb in natural rubidium is 2.591. Calculate the mass of 87Rb.arrow_forwardIn chemistry, what is meant by the term mole? What is the importance of the mole concept?arrow_forwardn chemistry, what is meant by the term mole? What is the importance of the mole concept?arrow_forward
- Use the periodic table shown in Fig. 4.9 to determine the atomic mass (per mole) or molar mass of each of the substances in column 1, and find that mass in column 2. l> Column 1 Column 2 (1) molybdenum (a) 33.99 g (2) lanthanum (b) 79.9 g (3) carbon tetrabromide (c) 95.94 g (4) mercury(II)oxide (d) l25.4g (5) titanium(iV) oxide (e) 138.9 g (6) manganese(ll) chloride (f) 143.1 g (7) phosphine, (g) 156.7 g (8) tin(II) fluoride (h) 216.6 g (9) lead(II) sulfide (i) 239.3 g (10) copper(I)oxide (j) 3316garrow_forwardhe “Chemistry in Focus” segment Plastic That Talks and Listens! discusses polyvinylidene difluoride (PVDF). What is the empirical formula of PVDF? Note: An empirical formula is the simplest whole-number ratio of atoms in a compound. This is discussed more fully in Sections 8.7 and 8.8 of your text.arrow_forwarderhaps the most important concept in introductory chemistry concerns what a mole of a substance represents. The mole concept will come up again and again in later chapters in this book. What does one mole of a substance represent on a microscopic, atomic basis? What does one mole of a substance represent on a macroscopic, mass basis? Why have chemists defined the mole in this manner?arrow_forward
- If one can find the ratio of the number of moles of the elements in a compound to one another, one can find the formula of the compound. In a certain compound of copper and oxygen, CuxOy, we find that a sample weighing 0.9573g contains 0.7649gCu. a. How many moles of Cu are there in the sample? (MolesofCu=massofCumolarmassofCu) _moles b. How many gram of O are there in the sample? The mass of the sample equals the mass of the Cu plus the mass of O. _g c. How many moles of O are there in the sample. _moles d. What is the mole ratio (molesofCu/molesofO) in the sample? _:1 e. What is the formula of the oxide? The atom ratio equals the mole ratio and is expressed using the smallest integers possible. _ f. What is the molar mass of the copper oxide? _g/molarrow_forwardUsing the average atomic masses given inside the front cover of this book, calculate the number of atoms present in each of the following samples. l type='a'> 1.50 g of silver, Ag 0.0015 moIe of copper, Cu 0.0015 g of copper, Cu 2.00 kg of magnesium, Mg 2.34 oz of calcium, Ca 2.34 g of calcium, Ca 2.34 moles of calcium, Caarrow_forwardFind the item in column 2 that best explains or completes the statement or question in column 1. l type="a"> Column 1 i>1 amu 1008 amu mass of the “average” atom of an element number of carbon atoms in 12.01 g of carbon 6.0221023 molecules total mass of all atoms in 1 mole of a compound smallest whole-number ratio of atoms present in a molecule formula showing actual number of atoms present in a molecule product formed when any carbon-containing compound is burned in O2 i>have the same empirical formulas, but different molecular formulas Column 2 msp;6.0221023 i>atomic mass mass of 1000 hydrogen atoms benzene, C6H6 , and acetylene, C2H2 i>carbon dioxide empirical formula 1.661023g i>molecular formula molar mass 1 molearrow_forward
- A jar contains some number of jelly beans. To find out precisely how many are in the jar, you could dump them out and count them. How could you estimate their number without counting each one? (Chemists need to do just this kind of bean counting when they work with atoms and molecules. Atoms and molecules are too small to count one by one, so chemists have worked out other methods to determine the number of atoms in a sample.)arrow_forwardYou find a compound composed only of element X and chlorine. and you know that the compound is 13.10% X by mass. Each molecule of the compound contains six times as many chlorine atoms as X atoms. What is element X?arrow_forwardYou find a compound composed only of element X and chlorine, and you know that it is 13.102% element X by mass. Each molecule has 6 times as many chlorine atoms as X atoms. What is element X?arrow_forward
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