111 T-Mobile? 6:16 PM × chapter six ONLINE HOMEWO… ? 106kj 5) 635 kJ Question 9
ID: 1044749 • Letter: 1
Question
111 T-Mobile? 6:16 PM × chapter six ONLINE HOMEWO… ? 106kj 5) 635 kJ Question 9 -16 60.0 mL of 0.350 M H2SO4 solution is mixed with 60.0 mL of 0.700 M NaOH solution in a coffee cup calorimeter of negligible heat capacity. The initial temperature of the two solutions are both at 23.0 degrees C. What is the final temperature? (What is the temperature change?) assume solutions have same specific heat and density as water. (s water 4.184 J/goC; d H20 = 1.00g/mL) H2504 + 2NaOH-> Na2SO4 + 2H2O ? Hrxn = 114 kj/mol rxn (1) 18.9 degrees C 2) 27.8 degrees C 3) 22.5 degrees C 2 of 12 completed Save for Later SubmitExplanation / Answer
moles of H2SO4 = 60 x 0.350 / 1000 = 0.021
moles of NaOH = 60 x 0.700 / 1000 = 0.042 mol
delta Hrxn = - 114 kJ/mol
H2SO4 + 2 NaOH ---------------> Na2SO4 + 2 H2O
1 2
0.021 0.042
Q = - n x deltaHrxn
= - 0.021 x 114
Q = 2.394 kJ
Q = m Cp dT
2394 = 120 x 4.184 x (Tf - 23)
Tf = 27.8
final temperature Tf = 27.8 oC
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.