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Two isotopes of gallium are naturally occurring, with Ga at 60.11% (68.93 amu) and Ga at 39.89% (70.92 amu). Calculate the atomic mass for gallium using the weighted 31 average mass method. Express your answer using four significant figures. amu Submit Request Answer

Two isotopes of gallium are naturally occurring, with Ga at 60.11% (68.93 amu) and Ga at 39.89% (70.92 amu). Calculate the atomic mass for gallium using the weighted 31 average mass method. Express your answer using four significant figures. amu Submit Request Answer

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Part A** Two isotopes of gallium are naturally occurring, with \(^{69}_{31}\text{Ga}\) at 60.11% (68.93 amu) and \(^{71}_{31}\text{Ga}\) at 39.89% (70.92 amu). Calculate the atomic mass for gallium using the weighted average mass method. **Express your answer using four significant figures.** [Input Box for Answer] amu [Submit Button] **Explanation:** To calculate the atomic mass of gallium: 1. Multiply the mass of each isotope by its relative abundance (as a decimal). 2. Sum these values to find the weighted average mass. \[ \text{Atomic Mass} = (68.93 \times 0.6011) + (70.92 \times 0.3989) \] Calculate and input the result in the provided box, ensuring it is to four significant figures.
Transcribed Image Text:**Part A** Two isotopes of gallium are naturally occurring, with \(^{69}_{31}\text{Ga}\) at 60.11% (68.93 amu) and \(^{71}_{31}\text{Ga}\) at 39.89% (70.92 amu). Calculate the atomic mass for gallium using the weighted average mass method. **Express your answer using four significant figures.** [Input Box for Answer] amu [Submit Button] **Explanation:** To calculate the atomic mass of gallium: 1. Multiply the mass of each isotope by its relative abundance (as a decimal). 2. Sum these values to find the weighted average mass. \[ \text{Atomic Mass} = (68.93 \times 0.6011) + (70.92 \times 0.3989) \] Calculate and input the result in the provided box, ensuring it is to four significant figures.
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