Respuesta :

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Answer:

The total amount of heat released  is  68.7 kJ

Explanation:

Given that:

mass of water = 94.0 g

moles of water = 94 / 18.02 = 5.216

80⁰C   ------>  0⁰C  -------->    -30⁰C

Q1 = m Cp dT

      = 94 x 4.184 x (0 - 80)

     = -31463.68 J

     = -31.43 kJ

Q2 = 6.01 x 10^3 x 5.216

    = - 31348.16 J

   = -31.35 kJ

Q3 = - 94 x 2.09 x 30

    = - 5893.8 J

   = -5.894 kJ

Total heat = Q1 + Q2 + Q3  = -31.43 kJ  + (-31.35 kJ  ) + (-5.894 kJ )  = -68.7 kJ

Total heat released = -68.7 kJ

Note that the "negative sign" simply indicates heat released, therefore no need to put it in the answer.

The total amount of heat released is 68.7 kJ.

Given:

Mass of water = 94.0 g

Moles of water = 94 / 18.02 = 5.216

Transformation of heat:

80⁰C   ------>  0⁰C  -------->   -30⁰C

Q₁ = m*Cp*dT

= 94 * 4.184 * (0 - 80)

= -31463.68 J

Q₁ = -31.43 kJ

Q₂ = 6.01 * 10³ * 5.216

= - 31348.16 J

Q₂ = -31.35 kJ

Q₃ = - 94 * 2.09 * 30

= - 5893.8 J

Q₃ = -5.894 kJ

Total heat = Q₁ + Q₂ + Q₃  

Total heat = -31.43 kJ  + (-31.35 kJ  ) + (-5.894 kJ )  = -68.7 kJ

Total heat = -68.7 kJ

Total heat released = -68.7 kJ

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