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kykrilka [37]
3 years ago
13

23.6 g of calcium chloride (110.98) is dissolved in water in a calorimeter. T rose from 25.0°C to 38.7°C. Heat capacity of solut

ion & calorimeter = 1258 J/°C. What is enthalpy change when 1 mol CaCl2 dissolves?
Chemistry
1 answer:
Soloha48 [4]3 years ago
5 0

Answer:

Enthalpy Change when 1 mole CaCl₂ dissolves

= - 81.13 kj/mole

Explanation:

Given information

    Mass of CaCl₂ = 23.6 g

Temperature changes from 25.0°C to 38.7°C

Heat capacity of solution & calorimeter (C) = 1258 J/°C

We know               Q = C x ΔT

                   ⇒ Heat released =  1258 x (38.7 - 25)

                                                = 1.7234 x 10⁴ J

                                                = 17.2 Kilo-joule

Thus 23.6 g is equivalent to 1.7234 x 10⁴ J or 17.2 Kilo-joule  of heat energy

Molar mass of calcium chloride (110.98)

Mole =\frac{Mass}{Molecular mass} = \frac{23.6}{110.98}  =0.212 mole

Enthalpy Change when 1 mole CaCl₂ dissolves

                      = \frac{-17.2}{0.212} kj/mol = -81.13 kj/mole

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Yakvenalex [24]

Answer:

T_2=-125.58\°C

Explanation:

Hello!

In this case, considering the Gay-Lussac's law which describes the pressure-temperature behavior as a directly proportional relationship by holding the volume as constant, we write:

\frac{T_1}{P_1} =\frac{T_2}{P_2}

Whereas solving for the final temperature T2, we get:

T_2=\frac{T_1P_2}{P_1}

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T_2=\frac{(22+273.15)K*1.75atm}{3.50atm} \\\\T_2=147.58K-273.15\\\\T_2=-125.58\°C

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