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Which element has a greater atomic mass A or B?
Element A has a greater atomic mass than element B if the atomic mass value of A is higher. The atomic mass represents the average mass of an element’s isotopes based on their abundance in nature.
What is the atomic mass of B if 19.9 percent of all B atoms have a mass of 10.01 amu and 80.1 percent have a mass of 11.01 amu?
Given : Atomic mass of B = 10.01 amu , % = 19.9 let it be A Atomic mass of B = 11.01 amu , % = 80.1 Solution : A and B are approximately in the ratio 1:4. Isotopic mass = [(proportion of A X at. mass of A) + (proportion of B X at. mass of B)] / 4 = [(1 X 10.01) + (4 X 11.01)] / 4 = (10.01 + 44.04) / 4 = 54.05 / 4 Isotopic atomic mass = 13.512 amu ---- Therefore, isotopic atomic mass of B is = 13.512 amu.
How do you calculate the atomic mas based on the number of protons and neutrons of an atom?
To calculate the atomic mass of an atom, you would add the number of protons and neutrons together. Protons and neutrons each have a mass of approximately 1 atomic mass unit (amu). The sum of the protons and neutrons will give you the atomic mass of the atom in atomic mass units.
If Element B Has 9 As The Atomic Number And 19 As The Mass Number What is The Answer how many protons does it have?
If Element B Has 9 As The Atomic Number And 19 As The Mass Number What is The Answer how many protons does it have?
What is the average atomic mass of an element with isotopes a b and c?
(mass of A) x (%of A) + (mass of B) x (% of B) + (mass of C) x (% of C)
The average atomic mass of boron is 10.81 amu. Based on the atomic mass of B-10 and the relative abundances of the boron isotopes what is the atomic mass of B-11?
The atomic mass of boron-11 (B-11) can be calculated by setting up an equation based on the given average atomic mass of boron and the known atomic mass and abundance of boron-10 (B-10). Since the average atomic mass is a weighted average of the isotopes, the equation would be: (mass of B-10 * % abundance of B-10) + (mass of B-11 * % abundance of B-11) = average atomic mass of boron. Solving this equation will give you the atomic mass of B-11.
Which element has a greater atomic mass A or B?
Element A has a greater atomic mass than element B if the atomic mass value of A is higher. The atomic mass represents the average mass of an element’s isotopes based on their abundance in nature.
What is the atomic mass of B if 19.9 percent of all B atoms have a mass of 10.01 amu and 80.1 percent have a mass of 11.01 amu?
Given : Atomic mass of B = 10.01 amu , % = 19.9 let it be A Atomic mass of B = 11.01 amu , % = 80.1 Solution : A and B are approximately in the ratio 1:4. Isotopic mass = [(proportion of A X at. mass of A) + (proportion of B X at. mass of B)] / 4 = [(1 X 10.01) + (4 X 11.01)] / 4 = (10.01 + 44.04) / 4 = 54.05 / 4 Isotopic atomic mass = 13.512 amu ---- Therefore, isotopic atomic mass of B is = 13.512 amu.
What is the average atomic mass of an element with isotopes a b c?
(mass of A) x (%of A) + (mass of B) x (% of B) + (mass of C) x (% of C)
What is average atomic mass of an element with isotopes A B and C?
(mass of A) x (%of A) + (mass of B) x (% of B) + (mass of C) x (% of C)
How do you calculate the atomic mas based on the number of protons and neutrons of an atom?
To calculate the atomic mass of an atom, you would add the number of protons and neutrons together. Protons and neutrons each have a mass of approximately 1 atomic mass unit (amu). The sum of the protons and neutrons will give you the atomic mass of the atom in atomic mass units.
What is the atomic mass rounded of boron?
Boron - B - Group IIIThe atomic number is 5.The mass number is 11.
If Element B Has 9 As The Atomic Number And 19 As The Mass Number What is The Answer how many protons does it have?
If Element B Has 9 As The Atomic Number And 19 As The Mass Number What is The Answer how many protons does it have?
What is the average atomic mass of an element with isotopes a b and c?
(mass of A) x (%of A) + (mass of B) x (% of B) + (mass of C) x (% of C)
What is the mass number of boron?
The mass number of boron is 11.
Which are true statements A There are 6.02 times 1023 particles in a moleB The mass of 1 mol is the same as the atomic mass in grams A mole weighs 6.02 times 1023 amu A mole is the atomic mass?
The true statements are A and B. Statement A is called Avogadro's number and represents the number of particles in one mole. Statement B refers to the molar mass, which is the mass of 1 mole of a substance expressed in grams, and is numerically equal to the atomic mass in atomic mass units (amu).
What changes in atomic number and mass number occur in beta emission?
Electron (beta minus) decay: the atomic mass remain approx. constant, the atomic number will be greater with 1 Positron (beta plus) and electron capture decay: the atomic mass remain approx. constant, the atomic number decrease with 1 Double beta decay: the atomic mass remain approx. constant, the atomic number will be greater with 2
