Question

1.

When a solid dissolves in water, heat may be evolved or
absorbed. The In the laboratory a general chemistry student finds that when 6.20 g of CsClO(s)
are dissolved in _{4}115.60 g of water, the
temperature of the solution drops from
22.87 to 19.50 °C.Based on the student's observation, calculate the enthalpy of dissolution of CsClO(s) in
kJ/mol._{4}Assume the specific heat of the solution is equal to the specific heat of water. ΔH _{dissolution} = kJ/mol2. |

When a solid dissolves in water, heat may be evolved or
absorbed. The
(dissolving) can be determined using a coffee cup
calorimeter.heat of dissolutionIn the laboratory a general chemistry student finds that when 20.92 g of BaBr(s)
are dissolved in _{2}111.60 g of water, the
temperature of the solution increases from
22.47 to 25.54 °C.Based on the student's observation, calculate the enthalpy of dissolution of BaBr(s) in
kJ/mol._{2}Assume the specific heat of the solution is equal to the specific heat of water. ΔH _{dissolution} = kJ/mol |

Answer #2

answered by: anonymous

When a solid dissolves in water, heat may be evolved or
absorbed. The heat of dissolution
(dissolving) can be determined using a coffee cup
calorimeter.
In the laboratory a general chemistry student finds that when
18.53 g of
Cs2SO4(s) are dissolved in
100.40 g of water, the temperature of the solution
drops from 25.54 to
22.92 °C.
The heat capacity of the calorimeter (sometimes referred to as the
calorimeter constant) was determined in a separate
experiment to be 1.85 J/°C....

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

The salt calcium bromide is soluble in water.
When 1.48 g of CaBr2
is dissolved in 112.00 g of water, the temperature
of the solution increases from 25.00 to
26.56 °C. Based on this observation, calculate the
enthalpy of dissolution of CaBr2 (in
kJ/mol).
Assume that the specific heat of the solution is 4.184 J/g °C and
that the heat absorbed by the calorimeter is negligible.
ΔHdissolution = kJ/mol

The salt cesium bromide is soluble in water.
When 9.28 g of CsBr is dissolved
in 115.00 g of water, the temperature of the
solution decreases from 25.00 to
22.72 °C. Based on this observation, calculate the
enthalpy of dissolution of CsBr (in kJ/mol).
Assume that the specific heat of the solution is 4.184 J/g °C and
that the heat absorbed by the calorimeter is negligible.
ΔHdissolution = kJ/mol

When a 5.93-g sample of solid sodium hydroxide dissolves in 39.8
g of water in a coffee-cup calorimeter (see above figure) the
temperature rises from 22.00 oC to 56.12 oC. Calculate H in kJ/mol
NaOH for the solution process. NaOH(s) Na+(aq) + OH-(aq) The
specific heat of water is 4.18 J/g-K.

When a 3.81-g sample of solid ammonium chloride dissolves in
57.9 g of water in a coffee-cup calorimeter (see above figure) the
temperature falls from 24.00 oC to 19.94 oC. Calculate H in kJ/mol
NH4Cl for the solution process. NH4Cl(s) NH4+(aq) + Cl-(aq) The
specific heat of water is 4.18 J/g-K.

When 7.56 g of NaCl is added to a coffee cup calorimeter, the
water temperature changes by 4.1 ºC. If the heat of solution (the
enthalpy change upon dissolving in water) is 3.8 kJ/mol, what mass
of solution must be in the cup? Assume the specific heat capacity
of the solution is the same as the specific heat capacity of
water.

When a 4.00-g sample of solid ammonium nitrate dissolves in 60.0
g of water in a coffee-cup calorimeter (see figure below), the
temperature drops from 23.0°C to 16.4°C. Calculate ΔH (in kJ/mol
NH4NO3) for the solution process shown below. Assume that the
specific heat of the solution is the same as that of pure water.
Hint: this process occurs at constant pressure.

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
solution be if it was initially at 25.0 °C? Assume that the heat
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
solute and solvent.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 2 minutes ago

asked 8 minutes ago

asked 9 minutes ago

asked 10 minutes ago

asked 14 minutes ago

asked 23 minutes ago

asked 28 minutes ago

asked 28 minutes ago

asked 30 minutes ago

asked 35 minutes ago

asked 37 minutes ago

asked 38 minutes ago