Naturally occuring boron is 80.20% boron-11 (atomic mass 11.01 amu) and 19.80% of some other isotope. What must the atomic mass of this second isotope be in order to account for the 10.81 amu average atomic mass of boron?.
1 answer:
You will have to do some math. <span>80.2 × 11.01 + 19.8 × x = 100 * 10.81. </span> <span>x is the mass in amu of the second isotope. </span> <span>Solve for x. </span> <span>19.8 × x = 100 * 10.81 - 80.2 × 11.01 </span> <span>19.8 × x = 1081 - 883.00 = 198.00 </span> <span>x = 1964.00 / 19.8 = 10.00 </span> <span>The mass of the other isotope is 10.00 amu.</span>
You might be interested in
The movement of rock pieces and other materials on earth's surface is called Weathering
Three that is the answer to your question
The answer is (1) 24. There are 26 protons in nucleus of Fe atom. There is 26 electrons in Fe atom. Fe atom loses 2 electrons and change to Fe2+ ion. So there is 24 electrons in Fe2+ ion.
Answer: The answer is Iceberg
Answer:
fgufyifyifyiyduhyufyiddjyfjyf86yif