an element X exists as two isotopes - 101 X and 104 X and weigh 100.95amu...
an element X exists as two isotopes - 101 X and 104 X and weigh 100.95amu and 103.95 amu, respectively. if the atomic weight of X is 102.67 amu, determine the percent abundance of the heavier isotope
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an element X exists as two isotopes - 101 X and 104 X and weigh
100.95amu...
The element lanthanum has an atomic weight of 139 and consists of two stable isotopes lanthanum-138...
The element lanthanum has an atomic weight of 139 and consists of two stable isotopes lanthanum-138 and lanthanum- 139. The isotope lanthanum-138 has a mass of 138 amu and a percent natural abundance of 8.90X10-2 %. The isotope lanthanum-139 has a percent natural abundance of 99.9%. What is the mass of lanthanum-1392 A certain element consists of two stable isotopes. The first has a mass of 113 amu and a percent natural abundance of 4.28 %. The second has a...
S A certain element exists as three natural isotopes as shown in the table below. Isotope...
S A certain element exists as three natural isotopes as shown in the table below. Isotope Mass (amu) Percent natural abundance 19.99244 90.51 20.99395 0.27 21.99138 9.22 Mass number 20 21 22 Calculate the average atomic mass of this element.
5. An element consists of two isotopes in the indicated natural abundances: Isotope A, mass=84.9118 amu,...
5. An element consists of two isotopes in the indicated natural abundances: Isotope A, mass=84.9118 amu, abundance = 72.15% Isotope B, mass = 86.9092 amu, abundance = 27.85% What is the atomic weight of this element? What is the identity of the element? Show your calculations.
An unknown element (Element X) has three naturally occurring isotopes. Complete the table by filling in...
An unknown element (Element X) has three naturally occurring isotopes. Complete the table by filling in the missing percent abundance (2 decimal places). Then calculate the atomic mass of element X (1 decimal place) and determine its identity by filling in its atomic symbol (case sensitive). Isotope Abundance (%) Atomic Mass (amu) 23.985042 1 78.99 2 24.985837 10.00 3 25.982593 amu Atomic mass of element X (1 decimal place): Atomic symbol of element X:
< Question 4 of 17 > Suppose that a fictitious element, X, has two isotopes: 59X...
< Question 4 of 17 > Suppose that a fictitious element, X, has two isotopes: 59X (59.015 amu) and "x (62.011 amu). The lighter isotope has an abundance of 75.7%. Calculate the average atomic mass of the element X average atomic mass:
A certain element consists of two stable isotopes. The first has an atomic mass of 34.9689...
A certain element consists of two stable isotopes. The first has an atomic mass of 34.9689 amu and a percent natural abundance of 75.53 %. The second has an atomic mass of 36.9474 amu and a percent natural abundance of 24.47 %. What is the atomic weight of the element? amu
QUESTION 3 A fictitious element is composed of isotopes A and B with masses of 61.9887...
QUESTION 3 A fictitious element is composed of isotopes A and B with masses of 61.9887 and 64.9846 amu respectively. The average atomic mass of the element is 64.52 amu. What can you conclude about the natural abundances of the two isotopes? O The natural abundance of isotope A must be greater than that of isotope B OThe natural abundance of isotope B must be greater than that of isotope A. O The natural abundances of both isotopes must be...
the element X has naturally occurring isotope. The masses (amu) and % abundance of the isotopes...
the element X has naturally occurring isotope. The masses (amu) and % abundance of the isotopes are given below. the average atomic mass of the element is ? Isotope: 221X, 220X, 218 X Abundance: 74.22, 12.78, 13.00 Mass: 220.9, 220.0, 218.1
The element carbon has two naturally occurring isotopes. The isotopic masses and abundances of these isotopes...
The element carbon has two naturally occurring isotopes. The isotopic masses and abundances of these isotopes are shown in the table below. Isotope 12c isotopic mass (amu) Abundance (%) 12.00 13.00 98.93 1.07 Calculate the average atomic mass of carbon to two digits after the decimal point. Number = _______ amu
If the mass of the only two isotopes of an element are 115.3026 amu and 122.8251...
If the mass of the only two isotopes of an element are 115.3026 amu and 122.8251 amu and the weighted average mass is 118.1471 amu, what is the percent abundance of the lighter isotope? Selected Answer: X b. 37.8 Correct Answer: e. 62.2
The element lanthanum has an atomic weight of 139 and consists of two stable isotopes lanthanum-138 and lanthanum- 139. The isotope lanthanum-138 has a mass of 138 amu and a percent natural abundance of 8.90X10-2 %. The isotope lanthanum-139 has a percent natural abundance of 99.9%. What is the mass of lanthanum-1392 A certain element consists of two stable isotopes. The first has a mass of 113 amu and a percent natural abundance of 4.28 %. The second has a...
S A certain element exists as three natural isotopes as shown in the table below. Isotope Mass (amu) Percent natural abundance 19.99244 90.51 20.99395 0.27 21.99138 9.22 Mass number 20 21 22 Calculate the average atomic mass of this element.
5. An element consists of two isotopes in the indicated natural abundances: Isotope A, mass=84.9118 amu, abundance = 72.15% Isotope B, mass = 86.9092 amu, abundance = 27.85% What is the atomic weight of this element? What is the identity of the element? Show your calculations.
An unknown element (Element X) has three naturally occurring isotopes. Complete the table by filling in the missing percent abundance (2 decimal places). Then calculate the atomic mass of element X (1 decimal place) and determine its identity by filling in its atomic symbol (case sensitive). Isotope Abundance (%) Atomic Mass (amu) 23.985042 1 78.99 2 24.985837 10.00 3 25.982593 amu Atomic mass of element X (1 decimal place): Atomic symbol of element X:
< Question 4 of 17 > Suppose that a fictitious element, X, has two isotopes: 59X (59.015 amu) and "x (62.011 amu). The lighter isotope has an abundance of 75.7%. Calculate the average atomic mass of the element X average atomic mass:
A certain element consists of two stable isotopes. The first has an atomic mass of 34.9689 amu and a percent natural abundance of 75.53 %. The second has an atomic mass of 36.9474 amu and a percent natural abundance of 24.47 %. What is the atomic weight of the element? amu
QUESTION 3 A fictitious element is composed of isotopes A and B with masses of 61.9887 and 64.9846 amu respectively. The average atomic mass of the element is 64.52 amu. What can you conclude about the natural abundances of the two isotopes? O The natural abundance of isotope A must be greater than that of isotope B OThe natural abundance of isotope B must be greater than that of isotope A. O The natural abundances of both isotopes must be...
The element carbon has two naturally occurring isotopes. The isotopic masses and abundances of these isotopes are shown in the table below. Isotope 12c isotopic mass (amu) Abundance (%) 12.00 13.00 98.93 1.07 Calculate the average atomic mass of carbon to two digits after the decimal point. Number = _______ amu
If the mass of the only two isotopes of an element are 115.3026 amu and 122.8251 amu and the weighted average mass is 118.1471 amu, what is the percent abundance of the lighter isotope? Selected Answer: X b. 37.8 Correct Answer: e. 62.2
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