Asap
1. ibuprofen (c13h18o2) is the active ingredient in many nonprescription pain relievers. each tablet contains 200 mg of ibuprofen, and a typical adult dose is two tablets every six hours.
• determine the molar mass of ibuprofen. show all steps to find the answer.
• calculate the number of moles of ibuprofen in a single tablet. show all steps to find the answer.
• calculate the number of moles of ibuprofen that an adult would have taken if she took four doses of ibuprofen in one day. show all steps to find the answer.

1) 206 g /mol

2) 0.971 mmol or 9.71 X 10⁻⁴ mol

3) 7.768 mmol or 7.768 X 10⁻³ mol

Explanation:

1) Let us calculate the molar mass by adding the atomic mass of each atom present in the given ibuprofen molecule.

Molecular formula : C₁₃H₁₈O₂

Molar mass = 13 X atomic mass of C + 18X atomic mass of H +2 X atomic mass of O

Molar mass = 13 X 12 + 18X1 + 2X16 = 206g/mol

2) moles is calculated as:

This is the moles in each ibuprofen tablet.

3) Now in each dose there are two tablets.

The adult took four doses

The number of tablets taken = 4X2 = 8

the number of moles taken = 8X0.971 mmol = 7.768 mmol

electron microscopy and scanning tunneling microscopes gives us a greater understanding of atoms by being able to see the atom itself, and lets us see some atomic reactions.

explanation:

the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.