Answer: A) 9.25 KJ.
B) - 148.296 KJ.
C) 296 KJ/mol.
Explanation:
For the reaction: S(s) + O2(g) β SO2(g), ΞH = -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 = ΞH 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 = ΞH 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 β9.25 KJ
B. The quantity of heat released when 0.501 mole of sulphur is burned in air is β148.296 KJ
C. The quantity of heat required to break 1 mole of SOβ is 296 KJ
S + Oβ β SOβ Β ΞH = β296 KJ/mol
From the balanced equation above,
32 g of S reacted to release β296 KJ/mol.
Therefore,
1 g of S will react to release = (1 Γ β296) / 32 = β9.25 KJ/mol
Thus, β9.25 KJ of heat energy is released
S + Oβ β SOβ Β ΞH = β296 KJ/mol
From the balanced equation above,
1 mole of S reacted to release β296 KJ/mol.
Therefore,
0.501 mole of S will react to release = 0.501 Γ β296 = β148.296 KJ/mol
Thus, β148.296 KJ of heat energy is released
SOβ β S + Oβ Β ΞH = 296 KJ/mol
From the balanced equation above,
296 KJ of heat is needed to break 1 mole of SOβ to its constituent.
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