Final answer:
C3H7NH3 can act as a Brønsted-Lowry acid because it is capable of donating a hydrogen ion (proton) to form its conjugate base in the presence of water.
Step-by-step explanation:
The molecule in question, C3H7NH3, can indeed function as a Brønsted-Lowry acid. The Brønsted-Lowry acid-base theory defines an acid as a substance that can donate a proton (H+ ion). The compound C3H7NH3 has a hydrogen atom that can be donated as a proton, making it an acid under this theory. To illustrate this, consider the compound in an aqueous solution:
C3H7NH3(aq) + H2O(l) → C3H7NH2(aq) + H3O+(aq)
C3H7NH3 is the chemical formula for a compound called propylamine. Propylamine (C3H7NH2) can act as a Brønsted-Lowry base by accepting a proton (H⁺ ion) from an acid to form its conjugate acid, C3H7NH3⁺. In this case, C3H7NH3⁺ is the conjugate acid, derived by the addition of a proton to the base (C3H7NH2) in a Brønsted-Lowry acid-base reaction.
Therefore, C3H7NH3 (propylamine in its protonated form) can act as a Brønsted-Lowry acid by donating a proton in suitable circumstances to form its conjugate base, C3H7NH2.