1. A volume of water was heated to 81.76 °C and immediately
added to 48.80 mL of water at 20.55 °C contained within a coffee
cup calorimeter. The final temperature of the mixture was 37.73 °C.
The final volume of water inside the calorimeter was 92.03 mL.
Assuming that them heat capacity of the solution is 4.18 J/g/°C,
calculate the following:
a. The volume of hot water added
ml
b. The mass of hot water (dwater = 1.00 g/mL)
g
c. The mass of the cold water (dwater = 1.00 g/mL)
g
d. The change in temperature (∆T) of hot water
°C
e. The change in temperature (∆T) of cold water
°C
f. The calorimeter constant in J/°C (Cp(water) = 4.18
J/g/°C)
J/°C
2. A 49.21 mL volume of 1.00 M HCl was mixed with 48.05 mL of 2.00
M NaOH in a coffee cup calorimeter (with calorimeter constant =
25.6 J/°C) at 20.32 °C. The final temperature of the aqueous
solution after the reaction was 29.83 °C. Assuming that them heat
capacity of the solution is 4.18 J/g/°C, calculate the
following:
a. The total mass of aqueous solution inside the calorimeter
(dsoln = 1.00 g/mL)
g
b. The change in temperature (∆T) of the aqueous solution
°C
c. The heat released by the neutralization reaction (this should be
a positive number)
J
d. The moles of HCl reacted
mol
e. The enthalpy change (∆H) for the neutralization in kJ/mol HCl (
this should be a negative number)
kJ/mol HCl
For the other answer please post it as another question......
1. A volume of water was heated to 81.76 °C and immediately added to 48.80 mL of water at 20.55 °C contained within a co...
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2. A 49.21 mL volume of 1.00 M HCl was mixed with 48.05 mL of 2.00 M NaOH in a coffee cup calorimeter (with calorimeter constant = 25.6 J/°C) at 20.32 °C. The final temperature of the aqueous solution after the reaction was 29.83 °C. Assuming that them heat capacity of the solution is 4.18 J/g/°C, calculate the following: a. The total mass of aqueous solution inside the calorimeter (dsoln = 1.00 g/mL) g correct 1/1 b. The change in...
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