Concept explainers
Interpretation:Mass law represented by the change should be illustrated
Concept introduction:Chemical compounds contain its constituent elements in a fixed ratio by mass and it is independent of its origin and the way of preparation, it is known as law of definite proportions.
For an isolated system, despite
If fixed mass of one component combine with different masses of second component to form more than one compound between them, then the ratios of masses of the second component that combine with the first component will be the ratios of simple whole numbers. This law is known as e law of multiple proportions.
Want to see the full answer?
Check out a sample textbook solutionChapter 2 Solutions
Principles of General Chemistry
- An element (A) has 5 isotopes. The masses (and abundances) of the isotopes 46A, 47A, 48A, 50A are 4595263 u (7.25 %), 46.9518 u (6.44 %), 47.9479 u (63.72 %), and 49.9448 u (5.18 %) respectively. If the element Ahas an atomic mass of 47.87 u, and the last isotope 49A has a percent abundance in the ratio of 3.361 that of SA, what is the mass of 49A?arrow_forwardState the mass law(s) demonstrated by the following experi-mental results, and explain your reasoning:Experiment 1: A student heats 1.00 g of a blue compound andobtains 0.64 g of a white compound and 0.36 g of a colorless gas.Experiment 2: A second student heats 3.25 g of the same bluecompound and obtains 2.08 g of a white compound and 1.17 g ofa colorless gasarrow_forwardA 2.540 g sample of an oxide of tin was heated in the air until the mass of the sample no longer changed, and 2.842 g of tin (IV) oxide (SnO2) was obtained as a result of the heating. b) What is the mass of tin in the final sample?arrow_forward
- A fictitious element is composed of isotopes A and B with masses of 61.9887and 64.9846 amu, respectively. The atomic mass of the element is 64.52. Whatcan you conclude about the natural abundances of the two isotopes?(a) The natural abundance of isotope A must be greater than the naturalabundance of isotope B.(b) The natural abundance of isotope B must be greater than the naturalabundance of isotope A.(c) The natural abundances of both isotopes must be about equal.(d) Nothing can be concluded about the natural abundances of the twoisotopes from the given information.arrow_forwardHydrogen sulfide is composed of two elements: hydrogen and sulfur. In an experiment, 6.500 g of hydrogen sulfide is fully decomposed into its elements. (a) If 0.384 g of hydrogen is obtained in this experiment, how many grams of sulfur must be obtained? (b) What fundamental law does this experiment demonstrate?arrow_forwardAtoms of the same type can have different mass numbers. These atoms are called "isotopes". Consider two electrically-neutral isotopes of carbon (C): . One carbon atom has a mass number of 12. One carbon atom has a mass number of 14. . (A) Which subatomic particle (protons, neutron, electron) do these two atoms have in common? How are they similar? (B) Which subatomic particle (protons, neutron, electron) is different among these two atoms? How are they different?arrow_forward
- The element oxygen has three naturally occurring isotopes, with 8,9, and 10 neutrons in the nucleus, respectively. (a) write the full chemical symbols for these three isotopes. (b) Describe the similarities and differences between the three kinds of atoms of oxygen.arrow_forwardThe element oxygen has three naturally occurring isotopes, with8, 9, and 10 neutrons in the nucleus, respectively. (a) Write thefull chemical symbols for these three isotopes. (b) Describethe similarities and differences between the three kinds ofatoms of oxygen.arrow_forward(1. On the second floor of Kent Laboratory a chemistry student in 111B finds that 15.20 g of nitrogen will react with 17.37 g, 34.74 g, or 43.43 g of oxygen to form three different compounds: (a) Calculate the ratio of the mass of oxygen to the mass of nitrogen for each compound and (b) Explain briefly how the numbers in part (a) support the atomic theory.arrow_forward
- It is common in mass spectrometry to assume that the massof a cation is the same as that of its parent atom. (a) Using datain Table 2.1, determine the number of significant figures thatmust be reported before the difference in masses of 1H and1H+ is significant. (b) What percentage of the mass of an 1Hatom does the electron represent?arrow_forwardThe natural abundance of the three stable isotopes are 90.92% isotope A (19.9924 amu),0.3104% isotope B (20.9938 amu), and 9.1784% isotope C (22.0330 amu). Calculate therelative (or average) atomic mass of this element and compare your value with that given inthe Periodic Table to identify the likely element. (Note: The units of atomic mass are atomicmass units (amu).arrow_forwardMagnesium has three isotopes with mass numbers 24, 25, and 26. (a) Write the complete chemical symbol (superscript andsubscript) for each. (b) How many neutrons are in an atom of each isotope?arrow_forward
- World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning