o 3/21/2018 11:55 PM O 5/103/16/2018 08:40 PM Gradebook Calculator- Periodic Tab
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o 3/21/2018 11:55 PM O 5/103/16/2018 08:40 PM Gradebook Calculator- Periodic Table Question 12 of 20 Sapling Learning In a constant-pressure calorimeter, 55.0 mL of 0.300 M Ba(OH)2 was added to 55.0 mL of 0.600 M HCI. The reaction caused the temperature of the solution to rise from 22.12 to 26.21 . If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/g·, respectively), what is dH for this reaction (per mole of H20 produced)? Assume that the total volume is the sum of the individual volumes. Number kJ/mol H,O Previous check AnswerNext Exit HintExplanation / Answer
Q = mcT
Q = heat energy (Joules, J), m = mass of a substance (kg)
c = specific heat (units J/kgK), is a symbol meaning "the change in"
T = change in temperature (Kelvins, K)
m = 55 + 55 = 110
T = 26.21 - 22.12 = 4.09 Deg Cel
Q = 110 x 4.184 x 4.09 = 1882.3816 Joules
Moles of water produced = 110 x 0.6 / 1000 = 0.066 Moles
Delta H = 2130.91 / 0.0374 x 1000 = 28.520 KJ
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