Respuesta :
The initial T is 25.0°C, and the specific heat capacity of the final solution is 3.50 J/g·K. The final T (temperature) is 51.2°C.
The standard enthalpy for H2SO4 (l) is -814 kJ/mole, whereas the standard enthalpy for H2SO4 (aq) is -909.3 kJ/mole.
Therefore, dHreaction = dHf (product) - dHf (reactant)
= -909.3 - (-814)
One mole of H2SO4 will be dissociated using the dHreaction, or q = -95.3 kJ of energy.
The formula, which may be used to calculate the heat change in calorimetry,
q = mass × specific heat capacity × temperature change —————- I
According to the information provided, H2SO4 has a density of 1.060 g/ml.
H2SO4 has a volume of 1 liter.
Therefore, density/volume = 1.060 g/ml / 1 103 ml = 1060 grams will be the mass of H2SO4.
Given that the starting point is 25.2°C or 273+25.2 = 298.2 K, let's assume the ending point is T2.
ΔT = T₂ -T₁ = T₂ - 298.2 K
Using the variables in the equation I we now obtain,
95.3 kJ = 1060 grams × 3.458 j/gK (T₂ - 298.2 K) (the specific heat capacity of the final solution is 3.458 J/gK)
(T₂ - 298.2 K) = 95300 J / 1060 × 3.458 = 26 K
T₂ = 298.2 K + 26 K
T2 is equal to 324.2 K, or 324.2 - 273 = 51.2 C.
Therefore, the final temperature(T) = 51.2 C.
To know more about specific heat capacity refer to: https://brainly.com/question/16952828
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