Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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1) Calculate the atomic mass of the isotopes 1H in grams (g). The atomic mass m1H = 1.007825 u. (Express your answer to five significant figures.)
2) Calculate the atomic mass of the isotopes 4He in grams (g). The atomic mass m4He = 4.002602 u. (Express your answer to five significant figures.)
3) Calculate the atomic mass of the isotopes 12C in grams (g). The atomic mass m12C = 12.000000 u. (Express your answer to five significant figures.)
4) Calculate the atomic mass of the isotopes 56Fe in grams (g). The atomic mass m56Fe = 55.934940 u. (Express your answer to five significant figures.)
5) Calculate the atomic mass of the isotopes 238U in grams (g). The atomic mass m238U = 238.050784 u. (Express your answer to five significant figures.)
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- An atom has a diameter of 2.50 Å and the nucleus of that atom has a diameter of 6.00 x 10-5 Å. Determine the fraction of the volume of the atom that is taken up by the nucleus. Assume the atom and the nucleus are a sphere. fraction of atomic volume: Calculate the density of a proton, given that the mass of a proton is 1.0073 amu and the diameter of a proton is 1.69 × 10-¹5 density: m. g/cm³arrow_forwardAn unmanned space shuttle mission brings samples back to Earth from Mars. Working with samples from mars, you discover that the isotope abundances on Mars are different from on Earth. You are tasked with calculating the average atomic mass (weight) of nitrogen that exists naturally on Mars. You find that the abundance of nitrogen-15 (atomic mass of 15.000 amu) on Mars is 11.639%, and the rest of the nitrogen (abundance = 100% - 11.639%) is nitrogen-14 (atomic mass 14.003 amu). Using that information, what is the average atomic mass (in amu) of nitrogen on Mars? (answer should have 3 decimal places - only input numbers, not "amu")arrow_forwardChromium which has an average atomic mass of 51.9961 amu has four isotopes. The masses of its isotopes are 49.94605 amu, 51.94051 amu, 52.94065 amu and 53.93888 amu. The first two isotopes have a total abundance of 87.87% and the last isotope has an abundance of 2.365%. What is the abundance of the third isotope? Answer textarrow_forward
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