A chimical reaction is supposed to produce 1.44 g of product X. When the reaction is carried out, only 1.31 g of product X are f
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Answer:
T₂ = 43.46 °C
Explanation:
Given that:
The heat of the formation of carbon dioxide = - 393.5 kJ/mol (Negative sign suggests heat loss)
It means that energy released when 1 mole of carbon undergoes combustion = 393.5 kJ = 393500 J
Heat gain by water = Heat lost by the reaction
Thus,
For water:
Mass of water = 5100 g
Specific heat of water = 4.18 J/g°C
T₁ = 25 °C
T₂ = ?
Q = 393500 J
So,
T₂ = 43.46 °C
The total heat of hydration of 1. 00 mol of gas phase ions and
ions is - 684 kJ/mol.
Calculation ,
Given data ,
Heat of solution = 17. 2 kJ/mol
lattice energy of KCl(s) = 701. 2 kJ/mol.
heat of hydration = ?
The KCl is formed by ions and
– ions
Δ = U° + Δ
Δ = Δ
- U° = 17. 2 kJ/mol - 701. 2 kJ/mol = - 684 kJ/mol
Hence, heat of hydration of 1. 00 mol of gas phase ions and
ions is - 684 kJ/mol.
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