An increase in water temperature is observed when 1.97 g of NaOH is added. The e
ID: 523545 • Letter: A
Question
An increase in water temperature is observed when 1.97 g of NaOH is added. The enthalpy change for this reaction is -2.19 kJ. Which of the statements is accurate?
The H°soln for NaOH is +44.5 kJ/mol so this is an endothermic process where energy in the form of heat is absorbed from the surroundings.
The H°soln for NaOH is -44.5 kJ/mol so this is an exothermic process where energy in the form of heat is released into the surroundings.
The H°soln for NaOH is -44.5 kJ/mol so this is an exothermic process where energy in the form of heat is absorbed from the surroundings
The H°soln for NaOH is +44.5 kJ/mol so this is an endothermic process where energy in the form of heat is absorbed from the surroundings.
The H°soln for NaOH is -44.5 kJ/mol so this is an exothermic process where energy in the form of heat is released into the surroundings.
The H°soln for NaOH is -44.5 kJ/mol so this is an exothermic process where energy in the form of heat is absorbed from the surroundings
Explanation / Answer
The Correct answer is
The H°soln for NaOH is -44.5 kJ/mol so this is an exothermic process where energy in the form of heat is released into the surroundings.
Molecular weight of NaOH = 40 g/mol
enthalpy change for a Mole = - 2.19 x 40 / 1.97 = -44.5 KJ/mol
The negative sign indicates that energy is released from system to surroundings
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