99% o Mobile 9:29 AM access1.lon-capa uiuc.edu C Logout CHEM 102F Fall 2014 I Ma
ID: 860551 • Letter: 9
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99% o Mobile 9:29 AM access1.lon-capa uiuc.edu C Logout CHEM 102F Fall 2014 I Main Menu Contents Grades Course Contents Exam 3 Timer Notes d Evaluate & Feedback Print You place a 100 mL of 0.50 M NaOH and 50 mL of 0.50 M HCl in a coffee cup calorimeter. What is the final temperature of the calorimeter if the initial temperature of the solution is 16.0 °C. (The change in enthalpy for the reaction is -55.4 kJ/mole H20) (assume the solution has specific heat and density as water, s 4.184 J/g oC, density 1.00 g/mL) 104.3 eV Submit Answer Incorrect. Tries 1/3 Tries Send FeedbackExplanation / Answer
Total Volume of solutions after mixing: 100 + 50 = 150 mL
d = 1.0 g/mL
Total Mass of solutions after mixing: d x V = 1.0 g/mL x 150 mL = 150 g
Heat released during neutralization = m x c x dT
Heat of neutralization given in terms of kJ/mol
Since the number of moles of acid and base is different;
n = M1 x V1 = (0.5 mol/L)(0.05 L) = 0.025 mole
Since -55.4 kJ of heat is released during the neutralization of 1 mol, for 0.025 mol the amount of heat : 1.385KJ = 1380.5 J
1380.5 = (150 g)(4.18 J/K.C)(T2 - 16)C
T2-16 = 2.201
T2= 18.201 0C
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