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The given question is incomplete. The complete question is:What is the relative atomic mass of a hypothetical element that consists isotopes in the indicated natural abundances.
Isotope mass amu Relative abundance
1 77.9 14.4
2 81.9 14.3
3 85.9 71.3
Express your answer to three significant figures and include the appropriate units.
Answer: 84.2 amu
Explanation:
Mass of isotope 1 = 77.9
% abundance of isotope 1 = 14.4% =
Mass of isotope 2 = 81.9
% abundance of isotope 2 = 14.3% =
Mass of isotope 3 = 85.9
% abundance of isotope 2 = 71.3% =
Formula used for average atomic mass of an element :
Therefore, the average atomic mass of a hypothetical element that consists isotopes in the indicated natural abundances is 84.2 amu
Answer:
a. 342.9 kJ of heat are absorbed.
Explanation:
Calculation of the moles of as:-
Mass = 20.00 g
Molar mass of = 17.031 g/mol
The formula for the calculation of moles is shown below:
Thus,
Given that:-
It means that 1 mole of undergoes reaction and absorbs 1168\ kJ of heat
So,
1168 mole of undergoes reaction and absorbs
of heat
<u>Amount of heat absorbed = + 342.9 KJ</u>