How many particles of LiClO4 are in 1.73 L of 2.40 M solution?

Sure, here are the steps to solve this problem:

1. First, we need to find out how many moles of LiClO4 are in 1.73 L of 2.40 M solution. The molarity (M) is defined as the number of moles of solute per liter of solution. So, we can calculate the number of moles by multiplying the volume of the solution by the molarity.

   Moles of LiClO4 = Volume (L) x Molarity (M) Moles of LiClO4 = 1.73 L x 2.40 mol/L = 4.152 moles

2. Next, we need to convert moles to particles. We can do this using Avogadro's number, which is 6.022 x 10^23 particles/mole.

   Particles of LiClO4 = Moles x Avogadro's number Particles of LiClO4 = 4.152 moles x 6.022 x 10^23 particles/mole = 2.50 x 10^24 particles

So, there are approximately 2.50 x 10^24 particles of LiClO4 in 1.73 L of 2.40 M solution.