SubmittedF3A sample of nitrogen has a mass of 42.1 grams.Submit Answer$a. How many N atoms are there in the sample?atomsb. How many N2 molecules are there in the sample?molecules[Review Topics][References]Use the References to access important values if needed for th%Retry Entire GroupF5Cengage Learning Cengage Technical Support5 more group attempts remainingF6&KF7*F8F9F10 3The compound NO2 can be formed by combining NO and O₂. This can be represented at the atomic level by a chemicalequation:EAccording to the law of conservation of mass, if 30.5 grams of NO and 16.3 grams of O₂ combine to form NO₂, howmany grams of NO2 must form?grams NO₂Submit AnswerC2NO+0₂ 2NO₂$4888F4RF→%5Retry Entire Group 9 more group attempts remainingCengage Learning Cengage Technical SupportTG6MacBook AirB17&7SYHUNtaht values if needed for this question.*8J1M(9KO)960LPEmail Instructor+AVPrevious Next>11BSave and Exitdelete

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[Review Topics] [References] Use the References to access important values if needed for th A sample of nitrogen has a mass of 42.1 grams. a. How many N atoms are there in the sample? atoms b. How many N2 molecules are there in the sample? molecules Submit Answer Retry Entire Group 5 more group attempts remaining

[Review Topics] [References] Use the References to access important values if needed for th A sample of nitrogen has a mass of 42.1 grams. a. How many N atoms are there in the sample? atoms b. How many N2 molecules are there in the sample? molecules Submit Answer Retry Entire Group 5 more group attempts remaining

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter10: The Mole

Section10.3: Moles Of Compounds

Problem 44PP

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An element X bas five major isotopes, which are listed below along with their abundances. What is the element? Isotope Percent Natural Abundance Mass (u) 46x 8.00% 45.95232 47x 7.30% 46.951764 48x 73.80% 47.947947 49x 5.50% 48.947841 50x 5.40% 49.944792
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) 3316g
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.)
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A diamond contains 5.0 1021 atoms of carbon. What amount (moles) of carbon and what mass (grams) of carbon are in ibis diamond?
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In chemistry, what is meant by the term mole? What is the importance of the mole concept?