Answer: A) 9.25 KJ.
B) - 148.296 KJ.
C) 296 KJ/mol.
Explanation:
For the reaction: S(s) + O2(g) → SO2(g), ΔH = -296 KJ/mol
A) The number of moles in 1.00 g of S is
n = mass/atomic mass = (1.00 g) / (32.00 g/mol) = 0.03125 mole
So, the quantity of heat when 1.00 g of sulfur burned in oxygen = ΔH of the reaction for 1.0 mole x no. of moles = (-296 KJ/mol) x (0.03125 mole) = 9.25 KJ.
B) The quantity of heat released when 0.501 mole of sulfur is burned in air = ΔH of the reaction for 1.0 mole x no. of moles = (-296 KJ/mol) x (0.501 mol) = - 148.296 KJ.
C) The quantity of energy is required to break up 1.0 mole of SO2(g) into its constituent elements = 296 KJ/mol.
It is the same that the amount of energy released when 1.0 mole of S is burned in oxygen.
The process of formation (burning of S) is exothermic.
On the other hand, the reverse operation (breakdown) must be endothermic (and therefore a positive energy change) = 296 KJ/mol.
A. The quantity of heat released when 1 g of sulphur is burned in oxygen is –9.25 KJ
B. The quantity of heat released when 0.501 mole of sulphur is burned in air is –148.296 KJ
C. The quantity of heat required to break 1 mole of SO₂ is 296 KJ
S + O₂ → SO₂ ΔH = –296 KJ/mol
From the balanced equation above,
32 g of S reacted to release –296 KJ/mol.
Therefore,
1 g of S will react to release = (1 × –296) / 32 = –9.25 KJ/mol
Thus, –9.25 KJ of heat energy is released
S + O₂ → SO₂ ΔH = –296 KJ/mol
From the balanced equation above,
1 mole of S reacted to release –296 KJ/mol.
Therefore,
0.501 mole of S will react to release = 0.501 × –296 = –148.296 KJ/mol
Thus, –148.296 KJ of heat energy is released
SO₂ → S + O₂ ΔH = 296 KJ/mol
From the balanced equation above,
296 KJ of heat is needed to break 1 mole of SO₂ to its constituent.
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