The atomic weight of Ga is 69.72 amu. There are 69.0 amu, and Ga, with a weight of 71.0 amu. The natural abundance of the Ga isotope is approximately: only two naturally occurring isotopes of gallium: 09 Ga, with a weight of 71

The atomic weight of Ga is 69.72 amu. There are 69.0 amu, and Ga, with a weight of 71.0 amu. The natural abundance of the Ga isotope is approximately: only two naturally occurring isotopes of gallium: 09 Ga, with a weight of 71

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...

See similar textbooks

Related questions

Q: A sample of chloroform is found to contain 12.0 g of carbon, 106.4 g of chlorine, and 1.01 g of…

A: Given : Mass of carbon in sample 1 = 12.0 g Mass of chlorine in sample 1 = 106.4 g Mass of hydrogen…

Q: the element silver has two naturally occurring isotopes. the mass of one isotope is 106.905 u and…

Q: Silver has two naturally isotopes and has an atomic mass of 107.868 amu. One isotope is Ag-109…

Q: Silver has an average atomic mass of 107.87 u. If 48.18% of Ag exists as Ag-109 (108.9047 u), what…

A: Given,average atomic mass of Ag = 107.87 u% abundance of Ag-109 = 48.18 %atomic mass of Ag-109 =…

Q: On earth, tin has 10 different stable isotopes. The heaviest, 124Sn makes up 5.80% of naturally…

A: Grams of 124Sn present in 38.3 g sample = 38.3*(5.80/100)= 2.22 g

Q: Naturally occurring chlorine (Cl) consists of two isotopes. One of the isotopes has a mass of 34.969…

A: Isotopes have same atomic number but different atomic mass or mass number. Atomic number is equal to…

Q: The metal magnesium consists of 3 isotopes with the following atomic masses and abundances: 24Mg -…

A: Given, 24Mg - 23.99 amu (78.70%) 25Mg - 24.99 amu (10.13%) 26Mg - 25.98 amu (11.17%).

Q: The proton mass is 1.007276 amu, the neutron mass is 1.008665 amu, and the electron mass is…

A: Given Mass of proton(mp) = 1.007276 amu Mass of electron(me) = 0.0005486 amu Mass of neutron(mn) =…

Q: An element has two isotopes. One isotope has a mass of 63.22g. The other has a mass of 67.88g. If…

Q: . An element has three stable isotopes with masses of 27.977 amu, 28,976 amu, and 29.973 amu. The…

Q: The atomic weight of Ga is 69.72 amu. There are only two naturally occurring isotopes of gallium: 69…

A: Given atomic weight of Ga is 69.72 amu

Q: In a sample of gallium there is 60.2% of gallium-69 (68.9 amu) atoms and 39.8% of gallium-71 (70.9…

Q: Potassium has 2 stable isotopes, 39K and 41K with atomic mass of 38.9637 amu and 40.9618 amu. If the…

A: Given: The average mass of potassium = 39.10 u The atomic mass of 39K = 38.9637 u The atomic mass…

Q: Calculate the weighted average of a substance from space. It has an abundance of 30.0% and 70.0% for…

A: The relative abundance definition in chemistry is the percentage of a particular isotope that occurs…

Q: On a certain planet two isotopes of indium can be found. The abundance of the isotope with a mass of…

A: We have the mass and abundance of two isotopes of indium. M1 = 114.9041 amup1 = 65.64 %M2 = 112.9043…

Q: 2. Bromine has two naturally occurring isotopes (Br-79 and Br-81) If the natural abundance of Br-79…

Q: In a naturally occurring sample, 19.8% of boron atoms have five neutrons and 80.2% have six…

Q: An unknown element has two naturally occurring isotopes. Isotope 1 has a mass of 119.0 amu and an…

A: Average mass of an element is defined as the atomic mass of the element calculated by multiplying…

Q: 5. A sample of Rb recovered from a nuclear reactor has an unusual distribution of isotopes. If the…

A: Average atomic mass is the sum of products of mass of each isotop and it’s natural abundance. It can…

Q: 2) Uranium is used in nuclear reactors and is a rare element on earth. Uranium has three common…

A: Step 1: Step 2: Step 3: Step 4:

Q: Q1* Rubidium has two naturally occurring isotopes, rubidium-85 (atomic mass=84.9118 amu;…

A: We have given the masses and isotopic abundance of three isotopes of rubidium. Isotopes of an…

Q: Bromine has two naturally occurring isotopes (Br-79 and Br-81) If the natural abundance of Br-79 is…

A: Given: There are two naturally occurring isotopes of Br. The abundance of isotope 1 = 50.69 % Mass…

Q: Copper, which has an average atomic mass of 63.546 amu, has two stable isotopes: copper-63 and…

A: Given,Atomic mass of Copper-63 = 63.546 amuAbundance of Copper-63= 69.15%

Q: An unknown element X has the following isotopes: 25X (80.50% abundant, mass = 25.03 amu) and 27X…

A: isotopes of X 25X: abundance - 80.50% (P1) = 80.50/100 = 0.8050 mass…

Q: uppose a new element is discovered and it has two stable isotopes. One isotope has a mass of 73.372…

A: When an element has more than one isotope, then we will take average atomic mass to calculate…

Q: Bromine has two naturally-occurring isotopes. 79Br has a mass of 78.9 amu and accounts for 58.3% of…

Q: An unknown element X has the following isotopes: ⁵²X (90.00% abundant), ⁴⁹X (8.00% abundant), ⁵⁰X…

A: The approximate atomic mass of element x is calculated as,

Q: Magnesium has three naturally occurring isotopes, 24Mg (isotopic mass = 23.9850 amu, abundance =…

A: Given data contains, Isotopic mass of 24Mg is 23.9850 amu. Abundance of 24Mg is 78.99%. Isotopic…

Q: An unknown element X has the following isotopes: 1ºX (20.00% abundant, atomic mass = atomic mass =…

Q: a) An element has two naturally occurring isotopes. Isotope l has a mass of 120.9038 u and a…

Q: Silver has just two naturally occuring isotopes: 107Ag with a fractional abundance of 0.51839 and…

A: Suppose the atomic mass of the most common isotope Ag107 is =y amu. It has a fractional abundance of…

Q: 7. Gallium has two naturally occurring isotopes. The mass of gallium-69 is 68.9256 amu and it is…

A: Average Atomic mass = (mass of 1st isotope x % abundance of 1st isotope + mass of 2nd isotope x %…

Q: An unknown element X has the following isotopes: ²⁵X (80.50% abundant, mass = 25.03 amu) and ²⁷X…

Q: A sample of gallium contains two isotopes and its atomic weight is 69.72 amu. If the sample is…

A: Isotopes can be defined as the members of same family having same atomic number but different mass…

Q: A sample of chloroform is found to contain 12.0 g of carbon, 106.4 g of chlorine, and 1.01 g of…

A: Total mass of chloroform in first sample = mass of C + mass of H + mass of Cl = (12.0+106.4+1.01) =…

Q: There are 2 isotopes of copper that occur naturally; 63Cu and 65Cu. The 63Cu atoms have a mass of…

A: PERCENT abundance for 63Cu is 69.717% PERCENT abundance for 65Cu is 30.283 %

Q: A particular element has 2 stable isotopes. If the first isotope has a mass of 14.754 amu and an…

A: Given that: Element has two stable isotope Mass of first isotope(m1) = 14.754amu Abundance of first…

Q: 6) Copper used in electric wires comes in two flavors (isotopes): "Cu and "Cu. "Cu has an atomic…

A: Average atomic mass of an atom can be calculated asAAM=100ma×abundancea+mb×abundanceb+.... We…

Q: Bromine has an average atomic mass of 79.904 amu. If Br-79 has a mass of 78.92 amu and Br-81 has a…

Q: Magnesium has three stable isotopes. The most commonly occurring isotope, 24Mg, has an isotopic mass…

A: Average atomic mass of an atom can be calculated using the mass of their isotopes and their…

Question

The atomic weight of Ga is 69.72 amu. There are
69.0 amu, and Ga, with a weight of 71.0 amu. The natural abundance of the Ga isotope is approximately:
only two naturally occurring isotopes of gallium: 09 Ga, with a weight of
71

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

Neon has three different isotopes. 90.51% of neon atoms have a mass of 19.992 amu. 0.27% of neon atoms have a mass of 20.994 amu. 9.22% of neon atoms have a mass of 21.991 amu. What is the average atomic mass of neon?
An unknown element X has the following isotopes: 52X (87.00% abundant), 49X (8.00% abundant), 50X (5.00% abundant). What is the approximate atomic mass of X?
Naturally occurring bromine is composed of two isotopes: 50.69 % Br-79 (mass of 78.9183 amu) and 49.31 % Br-81(mass of 80.9163 amu). Naturally occurring oxygen is composed of three isotopes: 99.757% O-16 (mass of 15.9949 amu), 0.038% O-17 (mass of 16.9991 amu), and 0.205% O-18 (mass of 17.9991 amu). The compound dibromonoxide is composed of two bromine atoms and one oxygen atom bonded together to form the Br2O molecule. Give the masses of the three most abundant Br2O molecules
If a fictitious element, X, has 2 naturally occurring isotopes; X-44 and X-46. The atomic mass of element X is known to be 45.31 amu, which isotope has the greatest natural abundance? Explain the reasoning for your choice.
Potassium has three isotopes with masses 38.9367 amu, 39.9640 amu, and 40.9618 amu. The abundance of the last isotope is 6.73%. Estimate the abundance of the other two isotopes
13) The element antimony has an atomic weight of 121.757 amu and only two naturally-occurring isotopes. One isotope has an abundance of 57.3% and an isotopic mass of 120.904 amu. Based on these data, what is the mass of the other isotope? a) 121.757 u b) 122.393 u c) 122.610 u d) 122.902 u
There are two naturally occurring isotopes of boron. 10B has a mass of 10.0129 u.11B has a mass of 11.0093 u. Determine the abundance of each isotope.
A hypothetical element has 3 stable isotopes. The masses of the isotopes and percent abundance of the first two isotopes are given. What is the percent abundance of Isotope 3? Isotope 1: 18.556 amu, 11.00% Isotope 2: 18.998 amu, 35.50% Isotope 3: 19.565 amu, ?
1) Antimony occurs in nature as a mixture of 2 isotopes. Sb-123 and Sb-121. If the Sb 121 has a mass of 120.9 amu and an abundance of 57.25%, and the average amu is 121.75, what is the abundance of the other isotope?
Consider the mass of Sulfur and Fluorine in compound A (16.6 g S, 9.80 g F) and compound B (23.2 g S, 55.0 g F). How do numbers like these support atomic theory?
Please show calculation
An element has three stable isotopes with masses of 27.977 amu, 28.976 amu, and 29.973 amu. The heavier two isotopes have an abundance of 4.68% and 3.09%, respectively. What is the mass of the element?