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
Right, let's go. For the atom ^16_6X: a) The atomic number of X is the subscript value. Z = 6 The atomic number is 6. b) The number of neutrons is the mass number minus the atomic number. Number of neutrons = A - Z = 16 - 6 = 10 The number of neutrons is 10. c) For a neutral atom, the number of electrons equals the atomic number. Number of electrons = Z = 6 The number of electrons is 6. d) The mass number of X is the superscript value. A = 16 The mass number is 16. If another atom is represented as ^18_8X, its relation to ^16_8X is that they are isotopes. Difference between ^16_8X and ^18_8X in terms of particles: • Both atoms have an atomic number of 8, meaning they both have 8 protons and 8 electrons. • They differ in their mass numbers: ^16_8X has a mass number of 16, while ^18_8X has a mass number of 18. • This difference in mass number is due to a difference in the number of neutrons. • For ^16_8X: Number of neutrons = 16 - 8 = 8. • For ^18_8X: Number of neutrons = 18 - 8 = 10. • Therefore, ^16_8X has 8 neutrons, and ^18_8X has 10 neutrons. To show that the relative atomic mass of X would be 16.2, given 90% of ^16_8X and 10% of ^18_8X: Step 1: Use the formula for relative atomic mass. Relative Atomic Mass (RAM) = (mass of isotope 1 × \% abundance 1) + (mass of isotope 2 × \% abundance 2)100 Step 2: Substitute the given values. RAM = ((16 × 90) + (18 × 10))/(100) Step 3: Calculate the products. RAM = (1440 + 180)/(100) Step 4: Sum the products and divide by 100. RAM = (1620)/(100) RAM = 16.2 The relative atomic mass of X is 16.2. Send me the next one 📸