Need help calculating the heat released into solution for the 3 reations
The Enthalpy Change of a Chemical ReactionExperiment 1The Enthalpy Change of a Chemical Reaction1. Record the following for each of the three trials:
· Trial 1
a | Mass of the empty calorimeter (g) 18.6g |
b | Initial temperature of the calorimeter (°C) 21.5°C |
c | Maximum temperature in the calorimeter from the reaction (°C) 35.0°C |
d | Calculate ΔT by subtracting (b) from (c) (°C) ΔT = T_{maximum} - T_{initial} _{35.0°C-21.5°C=13.5°C} |
e | Mass of the calorimeter and its contents after the reaction (g) 68.74g |
f | Calculate the mass of the contents of the calorimeter (g) by subtracting (a) from (e) 68.74g-18.6g=50.14g |
g | Calculate the moles of Mg reacted (MW = 24.305 g/mole) ? 50mL of 1M HCI is 50/1000x1=0.05 .15/24.305=.006g/mole |
· Trial 2
a | Mass of the empty calorimeter (g) 18.6g |
b | Initial temperature of the calorimeter (°C) 21.5°C |
c | Maximum temperature in the calorimeter from the reaction (°C) 44.0°C |
d | Calculate ΔT by subtracting (b) from (c) (°C) ΔT = T_{maximum} - T_{initial} _{44.0°C-21.5°C=22.5°C} |
e | Mass of the calorimeter and its contents after the reaction (g) 68.83g |
f | Calculate the mass of the contents of the calorimeter (g) by subtracting (a) from (e) 68.83-18.6=50.23 |
g | Calculate the moles of Mg reacted (MW = 24.305 g/mole) .25/24.305=.010g/mole |
· Trial 3
a | Mass of the empty calorimeter (g) 18.6g |
b | Initial temperature of the calorimeter (°C) 21.5°C |
c | Maximum temperature in the calorimeter from the reaction (°C) 52.9°C |
d | Calculate ΔT by subtracting (b) from (c) (°C) ΔT = T_{maximum} - T_{initial} _{52.9°C-21.5°C=31.4°C} |
e | Mass of the calorimeter and its contents after the reaction (g) 68.92g |
f | Calculate the mass of the contents of the calorimeter (g) by subtracting (a) from (e) 68.92g-18.6g=50.32 |
g | Calculate the moles of Mg reacted (MW = 24.305 g/mole) .35/24.305=.014g/mole |
2. Calculate the heat released into the solution for the 3 reactions, according to the formula:
q_{reaction}= (Ccal * ΔT) + (m_{contents}* Cp_{contents}* ΔT) |
Top Answer
1) Since the Ccal is not mentioned I will assume it to be zero Qreaction = m x Cp x dT ; Cp for water based systems is 4.18... View the full answer