A chemist must dilute of aqueous copper(II) sulfate solution until the concentration falls to . He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Be sure your answer has the correct number of significant digits.

The final volume of the copper (ii) sulfate solution = 93.6 mL

Note: The question is incomplete. The complete question is given below:

A chemist must dilute 37.0 mL of 602. mM aqueous copper(II) sulfate (Cuso4) solution until the concentration falls to 238. mM. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Be sure your answer has the correct number of significant digits.

Explanation:

Using the equation of dilution, C₁V₁ = C₂V₂

where C₁ = initial concentration

V₁ = initial volume

C₂ = final concentration

V₂ = final volume

For the aqueous solution of copper (ii) sulfate

C₁ = 602 mM; V₁ = 37.0 mL; C₂ = 238 mM; V₂ = ?

Making V₂ subject of formula

V₂ = C₁V₁/C₂

V₂ = (602 mM * 37.0 mL)/238 mM

V₂ = 93.6 mL

Therefore, the final volume of the copper (ii) sulfate solution = 93.6 mL

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :