q=4.184 J/(gC) * 50.15g * 8.27C=1735 J
q=4.184 J/((gC) * 50.25g * 13.78 C= 2897 J
q=4.184 J/(gC) * 50.35 g * 19.29 C= 4064 J
I need help with Part 2
Part 1. Record the following for each of the three experiments:
(a) Mass of the empty calorimeter (g): 11.600 g
(b) Initial temperature in the calorimeter (C): 21.00
(c) Maximum temperature in the calorimeter from the reaction (C): 29.27, 34.78, 40.29
(d) Calculate deltaT as Tmaximum - Tinitial (C): 8.27, 13.78, 19.29
(e) Mass of the calorimeter and its contents after the reaction (g): 61.557g, 61.649g, 61.741g
(f) Calculate the mass of the contents of the calorimeter (g): 49.957g, 50.049g, 50.141g
(g) Calculate the moles of Mg reacted (MW=24.305 g/mole): 3.645, 6.076, 8.506 or the moles can be 0.006, .103, .014
**Part 2**. Calculate the heat released into the solution for the 3 reactions, according to:
q(reaction) = Ccal * Delta T + mass(contents) * Cp (contents) * deltaT
2 answers
Hey amanda what was the correct answer for g
3 answers