To what volume should you dilute 122 mL of an 8.20 M CuCl2 solution so that 51.0 mL of the diluted solution contains 4.40 g CuCl2

The first thing to do here is to use the molarity and the volume of the initial solution to figure out how many grams of copper(II) chloride it contains.133mL solution⋅1L103mL⋅7.90 moles CuCl21L solution=1.051 moles CuCl2To convert this to grams, use the compound's molar mass1.051moles CuCl2⋅134.45 g1mole CuCl2=141.31 g CuCl2Now, you know that the diluted solution must contain 4.49 g of copper(II) chloride. As you know, when you dilute a solution, you increase the amount of solvent while keeping the amount of solute constant.This means that you must figure out what volume of the initial solution will contain 4.49 g of copper(II) chloride, the solute.4.49g⋅133 mL solution141.32g=4.23 mL solution−−−−−−−−−−−−−− The answer is rounded to three sig figs.You can thus say that when you dilute 4.23 mL of 7.90 M copper(II) chloride solution to a total volume of 51.5 mL , you will have a solution that contains 4.49 g of copper(II) chloride.

Spontaneity tell us the direction of the reaction, but not how fast it goes. gibbs free energy brings together enthalpy, entropy and temperature in one easy formula. g = h - ts. and, finally the sign of delta g is always negative for a spontaneous reaction.