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? Paired item 1)
A) 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.
B) 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.
C) 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.
Correct Answer:
Verified
Q7: A reaction where the products are higher
Q8: Bomb calorimetry is carried out at _.
Q9: Given the ∆H°f, calculate the ∆H°rxn for
Q10: If ΔH = -54.74 kJ for a
Q12: A drop in water temperature is observed
Q14: A _ is an experimental set-up that
Q15: You are asked to design an experiment
Q16: A chemical reaction that gives off energy
Q45: An _ reaction results when the energy
Q56: An _ reaction results when the energy
Unlock this Answer For Free Now!
View this answer and more for free by performing one of the following actions
Scan the QR code to install the App and get 2 free unlocks
Unlock quizzes for free by uploading documents