This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Step 1: Understand the formula for relative atomic mass. The relative atomic mass (Ar) of an element is the weighted average of the mass numbers of its isotopes, taking into account their natural abundances. For two isotopes, the formula is: Ar = (mass number of isotope 1 × abundance of isotope 1) + (mass number of isotope 2 × abundance of isotope 2) The abundances are usually expressed as decimals (percentage divided by 100). Step 2: Identify the given values. Relative atomic mass of Q (Ar_Q) = 14.0037 Isotope 1: ^15Q Mass number of isotope 1 = 15 Abundance of isotope 1 = 0.37% = (0.37)/(100) = 0.0037 Isotope 2: Let its mass number be x. Abundance of isotope 2 = ? Step 3: Calculate the abundance of the second isotope. Since there are only two isotopes, their abundances must sum to 100%. Abundance of isotope 2 = 100% - Abundance of isotope 1 Abundance of isotope 2 = 100% - 0.37% = 99.63% As a decimal, abundance of isotope 2 = (99.63)/(100) = 0.9963 Step 4: Substitute the values into the relative atomic mass formula and solve for x. 14.0037 = (15 × 0.0037) + (x × 0.9963) 14.0037 = 0.0555 + 0.9963x Subtract 0.0555 from both sides: 14.0037 - 0.0555 = 0.9963x 13.9482 = 0.9963x Divide by 0.9963: x = (13.9482)/(0.9963) x = 14.0000 The mass number must be a whole number. The mass number of the second isotope is 14. 3 done, 2 left today. You're making progress.