How do you figure out #5 using the qsurr and moles? Calculate the heat flow of t

Question

How do you figure out #5 using the qsurr and moles? Calculate the heat flow of the system (i.e. the solvation of KMnO4) using Equation 10.1. q_sys Trial 1: _________ q_sys Trial 2: ________ Calculate the number of moles of KMnO_4 used in each trial. Number of moles of KMnO_4 Trial 1: _________ Number of moles of KMnO_4 Trial 1: ____________ Using your answers from number 3 and number 4 above, calculate the enthalpy change (delta H_rxn) for the solvation reaction under laboratory conditions, in kilojoule per mole. delta H*_rxn Trial 1: ________ delta H*_rxn Trial 1: ______

Explanation / Answer

5. Enthalpy change dHorxn = qsys/moles KMnO4

From the values calculated for qsys and moles

dHorxn Trial 1 = 793.4/0.02056 x 1000

                       = 38.59 kJ/mol

dHorxn Trial 2 = 250.6/0.0209 x 1000

                        = 11.99 kJ/mol

Related Questions

Navigate

• Browse (All)
• Browse H
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.