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Answer:
The enthalpy change for the solution process = - 158.34 kJ/mol
Explanation:
Given that:
The mass of salt AX = 2.499 g
The mass of water = 135.3 g
The mass of the solution = ( 2.499 + 135.3 ) g = 137.799 g
The specific heat of salt solution s is known to be = 4.18 J/g° C
The change in temperature i.e. ΔT = 35.2 °C - 23.6 °C = 11.6 °C
Thus, the amount of heat raised is equal to the heat absorbed by the calorimeter.
∴
Recall that the mass of the salt = 2.499 g
The number of moles of the salt =
= 0.0422 mol of AX
Finally the enthalpy change,
= - 158.34 kJ/mol
The enthalpy change for the solution process = - 158.34 kJ/mol
Answer:
The concentration of the most dilute solution is 0.016M.
Explanation:
First, a solution is prepared and then it undergoes two subsequent dilutions. Let us calculate initial concentration:
<u>First dilution</u>
We can use the dilution rule:
C₁ x V₁ = C₂ x V₂
where
Ci are the concentrations
Vi are the volumes
1 and 2 refer to initial and final state, respectively.
In the first dilution,
C₁ = 0.178 M
V₁ = 15 mL
C₂ = unknown
V₂ = 50 mL
Then,
<u>Second dilution</u>
C₁ = 0.053 M
V₁ = 15 mL
C₂ = unknown
V₂ = 50 mL
Then,