If the solubility of a gas is 8.4 g/L at 404 kPa pressure, what is the solubility of the gas when the pressure is 101 kPa? Pleas
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<u>Answer:</u> The enthalpy change of the reaction is -243 J/mol
<u>Explanation:</u>
The heat released by the reaction is absorbed by the calorimeter and the solution.
The chemical equation used to calculate the heat released follows:
where,
c = heat capacity of calorimeter = 1620 J/K
= change in temperature =
(Change remains same)
Putting values in above equation, we get:
<u>Sign convention of heat:</u>
When heat is absorbed, the sign of heat is taken to be positive and when heat is released, the sign of heat is taken to be negative.
For the given chemical reaction:
We are given:
Moles of monoclinic sulfur = 1 mole
- To calculate the enthalpy change of the reaction, we use the equation:
where,
q = amount of heat released = -243 J
n = number of moles = 1 mole
= enthalpy change of the reaction
Putting values in above equation, we get:
Hence, the enthalpy change of the reaction is -243 J/mol
Calcium oxide (CaO) or lime in solid form can be prepared from the decomposition of calcium hydroxide {Ca in to lime (CaO) and water (
at high temperature. The reaction is an endothermic reaction. That is heat is absorbed in this reaction process. One mole of calcium hydroxide decomposed into one mole of calcium oxide and one mole of water. The balanced reaction can be shown as-CaC
(solid) → CaO (solid) +
(liquid). The heat of the reaction is (+) 63.7 kJ/mole of CaO.