Question

Given the data in the table below, what is the enthalpy of dissolution of KOH? The molar mass of KOH is 56.11 g/mol, the specific heat of solution is 4.184 J/gºC, and the calorimeter constant is 22.45 J/ºC. To receive full points for this question, list every step of your calculation.

mass of water added to the calorimeter 50.000 g

initial temperature of the water 22.0 ºC

mass of KOH added to the calorimeter 1.824 g

final temperature in the calorimeter 29.9 ºC

Answer #1

Compute for the enthalpy (heat) of dissolution of a salt
(NH4Cl) in Joules using the following data:
Mass of salt, g = 5.00
Mass of calorimeter, g = 5.10
Mass of calorimeter + water, g = 30.204
Initial Temperature, °C = 25.35
Final Temperature. °C = 17.19
Use the following:
MWNH4Cl = 53.5 g/mol
Specific HeatNH4Cl = 1.57 J/g·°C

The enthalpy change for the dissolution of NH4NO3 is +26.8
kJ/mol. When 40.0 g of NH4NO3 dissolves in 250.0 g of water in a
coffee cup calorimeter, what will the final temperature of a
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capacity of the solution is the same as the specific heat of pure
water, 4.184 J/(g·K). Hint: don't forget to add the masses of
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When a solid dissolves in water, the solution may become hotter
or colder. The dissolution enthalpy (dissolving) can be determined
using a coffee cup calorimeter. In the laboratory a general
chemistry student finds that when 10.13 g K2SO4(s) is dissolved in
114.80 g water, the temperature of the solution drops from 24.11 to
20.86 °C. The heat capacity of the calorimeter (sometimes referred
to as the calorimeter constant) was determined in a separate
experiment to be 1.77 J/°C. Based on...

A student determines the heat of dissolution of solid
ammonium bromide using a coffee-cup calorimeter of
negligible heat capacity.
When 6.34 g of
NH4Br(s) is dissolved in
119.00 g of water, the temperature of the solution
drops from 25.00 to 22.76 °C.
Based on the student's observation, calculate the enthalpy of
dissolution of NH4Br(s) in kJ/mol.
Assume the specific heat of the solution is 4.184 J/g°C.
ΔHdissolution = kJ/mol

An object with a specific heat of 0.800 J/gºC at a temperature
of 405 ºC is placed in a calorimeter with a heat capacity of 2.00
J/ºC that contains 100.0 mL of water. The initial temperature of
the water and the calorimeter is 25.3ºC. After the object is added
to the calorimeter, the final temperature of the calorimeter,
water, and object is 29.8ºC. What is the mass of the object in
grams?

coffee cup calorimeter contained 50.0 mL of a 1.33 M KOH
solution at an initial temperature of 23.3 ºC. A student quickly
add 40.0 mL of 1.54 M HNO3 to the calorimeter. The
maximum temperature reached during the neutralization reaction was
29.1ºC.
assume specific heat of solution is the same as specific heat of
water = 4.18 J/gºC
assume density of both KOH and HNO3 are the same as
water = 1.00 g/mL
_________________________________________________________________
This is more of a question...

If 3.403 g KOH are dissolved in 100.327 g H2O and the
temperature increases by 4.28 oC, the enthalpy of dissolution of
KOH in water is ___ kJ/mol. Assume the specific heat of the
resulting KOH solution is 4.18 J g-1oC-1.

When 10.0 g KOH is dissolved in 100.0 g of water in a coffee-cup
calorimeter, the temperature rises from 25.18 ˚C to 47.53 ˚C.
Calculate the ∆Hrxn for the dissolution process. Assume that the
solution has a specific heat capacity of 4.184 J/gK

How does the temperature and specific heat capacity of a sample
of water (the calorimeter) change as a different mass or
temperature of hot metal is added to it?
How does the temperature and specific heat capacity of a sample
of water (the calorimeter) change as the volume of water is
changed?
How does the molar enthalpy of dissolution change with the
amount of substance added to water?
How does the molar enthalpy of dissolution change with the
volume of...

A 1.000 g sample of octane (C8H18) is burned in a bomb
calorimeter containing 1200 grams of water at an initial
temperature of 25.00ºC. After the reaction, the final temperature
of the water is 33.20ºC. The heat capacity of the calorimeter (also
known as the “calorimeter constant”) is 837 J/ºC. The specific heat
of water is 4.184 J/g ºC. Calculate the heat of combustion of
octane in kJ/mol.

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