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: State the formula for relative atomic mass. The relative atomic mass of an element with multiple isotopes is calculated using the formula: Relative Atomic Mass = (mass of isotope × fractional abundance of isotope) For two isotopes, this becomes: Relative Atomic Mass = (A_1 × P_1) + (A_2 × P_2) where A_1 and A_2 are the mass numbers of the isotopes, and P_1 and P_2 are their respective fractional abundances. Step 2: Determine the abundance of the second isotope. Given that element Q has two isotopes and the abundance of the first isotope (P_1) is 99.63\%. The sum of the abundances of all isotopes must be 100\%. P_1 + P_2 = 100\% 99.63\% + P_2 = 100\% P_2 = 100\% - 99.63\% = 0.37\% Convert percentages to fractional abundances: P_1 = (99.63)/(100) = 0.9963 P_2 = (0.37)/(100) = 0.0037 Step 3: Substitute the known values into the relative atomic mass formula. Given: Relative Atomic Mass of Q = 14.0037 Mass number of the first isotope (A_1) = 14 Abundance of the first isotope (P_1) = 0.9963 Abundance of the second isotope (P_2) = 0.0037 Let the mass number of the second isotope be A_2. 14.0037 = (14 × 0.9963) + (A_2 × 0.0037) Step 4: Solve for A_2. 14.0037 = 13.9482 + (A_2 × 0.0037) Subtract 13.9482 from both sides: 14.0037 - 13.9482 = A_2 × 0.0037 0.0555 = A_2 × 0.0037 Divide by 0.0037: A_2 = (0.0555)/(0.0037) A_2 = 15 The mass number of an isotope must be a whole number. The mass number of the second isotope is 15. Send me the next one 📸