a. Using the average atomic mass of carbon, calculate the mass (in amu) of 138 carbon atoms.amub. Using the average atomic mass of potassium, calculate the mass (in amu) of 6.60 x 106 potassium atoms.c. Using the average atomic mass of lithium, calculate the mass (in amu) of 8.60 x 1023 of lithium atoms.amuSubmit Answerd. Using the average atomic mass of magnesium, calculate the mass (in amu) of 5 magnesium atoms.amue. Using the average atomic mass of iodine, calculate the mass (in amu) of 3.300 x 1023 iodine atoms.Show HintamuamuRetry Entire Group9 more group attempts remainingPreviousNextSave and Exit

Note: As per the guidelines solution of 1st question has been made. For the expert solution of…

a. Using the average atomic mass of carbon, calculate the mass (in amu) of 138 carbon atoms. amu b. Using the average atomic mass of potassium, calculate the mass (in amu) of 6.60 x 106 potassium atoms. amu c. Using the average atomic mass of lithium, calculate the mass (in amu) of 8.60 x 1023 of lithium atoms. amu d. Using the average atomic mass of magnesium, calculate the mass (in amu) of 5 magnesium atoms. amu e. Using the average atomic mass of iodine, calculate the mass (in amu) of 3.300 x 1023 iodine atoms. amu

a. Using the average atomic mass of carbon, calculate the mass (in amu) of 138 carbon atoms. amu b. Using the average atomic mass of potassium, calculate the mass (in amu) of 6.60 x 106 potassium atoms. amu c. Using the average atomic mass of lithium, calculate the mass (in amu) of 8.60 x 1023 of lithium atoms. amu d. Using the average atomic mass of magnesium, calculate the mass (in amu) of 5 magnesium atoms. amu e. Using the average atomic mass of iodine, calculate the mass (in amu) of 3.300 x 1023 iodine atoms. amu

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter2: Atoms, Molecules, And Ions

Section: Chapter Questions

Problem 43E: Early tables of atomic weights (masses) were generated by measuring the mass of a substance that...

See similar textbooks

Similar questions

Reference Section 5-2 to find the atomic masses of 12C and 13C, the relative abundance of 12C and 13C in natural carbon, and the average mass (in u) of a carbon atom. If you had a sample of natural carbon containing exactly 10,000 atoms, determine the number of 12C and 13C atoms present. What would be the average mass (in u) and the total mass (in u) of the carbon atoms in this 10,000-atom sample? If you had a sample of natural carbon containing 6.0221 1023 atoms, determine the number of 12C and 13C atoms present What would be the average mass (in u) and the total mass (in u) of this 6.0221 1023 atom sample? Given that 1 g = 6.0221 1023 u, what is the total mass of I mole of natural carbon in units of grams?
The element europium exists in nature as two isotopes: 151Eu has a mass of 150.9196 u and 153Eu has a mass of 152.9209 u. The average atomic mass of europium is 151.96 u. Calculate the relative abundance of the two europium isotopes.
The element silver (Ag) has two naturally occurring isotopes: 109 Ag and 107Ag with a mass of 106.905 u. Silver consists of 51.82% 107Ag and has an average atomic mass of 107.868 u. Calculate the mass of 109Ag.
Early tables of atomic weights (masses) were generated by measuring the mass of a substance that reacts with 1.00 g of oxygen. Given the following data and taking the atomic mass of hydrogen as 1.00, generate a table of relative atomic masses for oxygen, sodium, and magnesium. Element Mass That Combines with 1.00g Oxygen Assumed Formula Hydrogen 0.126 g HO Sodium 2.875 g NaO Magnesium 1.500 g MgO How do your values compare with those in the periodic table? How do you account for any differences?
Indium oxide contains 4.784 g of indium for every 1.000 g of oxygen. In 1869, when Mendeleev first presented his version of the periodic table, he proposed the formula In2O3 for indium oxide. Before that time it was thought that the formula was InO. What values for the atomic mass of indium are obtained using these two formulas? Assume that oxygen has an atomic mass of 16.00.
These questions concern the work of J. J. Thomson: From Thomson’s work, which particles do you think he would feel are most important in the formation of compounds (chemical changes) and why? Of the remaining two subatomic particles, which do you place second in importance for forming compounds and why? Come up with three models that explain Thomson’s findings and evaluate them. To be complete you should include Thomson’s findings.
There are 1.699 1022 atoms in 1.000 g of chlorine. Assume that chlorine atoms are spheres of radius 0.99 and that they are lined up side by side in a 0.5-g sample. How many miles in length is the line of chlorine atoms in the sample?
The average atomic masses of some elements may vary, depending upon the sources of their ores. Naturally occurring boron consists of two isotopes with accurately known masses ( 10B, 10.0129 amu and 11B, 11.0931 amu). The actual atomic mass of boron can vary from 10.807 to 10.8 19, depending on whether the mineral source is from Turkey or the United States. Calculate the percent abundances leading to the two values of the average atomic masses of boron from these two countries.
A cube of sodium has length 1.25 in. How many atoms are in that cube? (Note: dNa=0.968 g/cm3.)
Copper: (a) Suppose you have a cube of copper metal that is 0.236 cm on a side with a mass of 0.1206 g. If you know that each copper atom (radius = 128 pm) has a mass of 1.055 1022 g (you will learn in Chapter 2 how to find the mass of one atom), how many atoms are there in this cube? What fraction of the cube is filled with atoms? (Or conversely, how much of the lattice is empty space?) Why is there empty space in the lattice? (b) Now look at the smallest, repeating unit of the crystal lattice of copper. Knowing that an edge of this cube is 361.47 pm and the density of copper is 8.960 g/cm3, calculate the number of copper atoms in this smallest, repeating unit.
The following chart shows a general decline in abundance with increasing mass among the first 30 elements. The decline continues beyond zinc. Notice that the scale on the vertical axis is logarithmic, that is, it progresses in powers of 10. The abundance of nitrogen, for example, is 1/10,000 (1/104) of the abundance of hydrogen. All abundances are plotted as the number of atoms per 102 atoms of H. (The fact that the abundances of Li, Be, and B, as well as those of the elements near Fe, do not follow the general decline is a consequence of the way that elements are synthesized in stars.) (a) What is the most abundant main group metal? (b) What is the most abundant nonmetal? (c) What is the most abundant metalloid? (d) Which of the transition elements is most abundant? (e) Which halogens are included on this plot, and which is the most abundant?
When a sample of phosphorus burns in air, the compound P4O10 forms. One experiment showed that 0.744 g of phosphorus formed 1.704 g of P4O10. Use this information to determine the ratio of the atomic weights of phosphorus and oxygen (mass P/mass O). If the atomic weight of oxygen is assumed to be 16.000, calculate the atomic weight of phosphorus.