Question

A student dissolves 10. g of sodium carbonate in a coffee cup calorimeter and measures an increase in water temperature of 2.3 degrees. Assuming the coffee cup contained 175 g of pure water, what is the ΔH of solution for this reaction in kJ/mol?

Answer #1

thanks and hope you like the answer

A student dissolves 10. g of sodium carbonate in a coffee cup
calorimeter and measures an increase in water temperature of 8.0
degrees. Assuming the coffee cup contained 175 g of pure water,
what is the ΔH of solution for this reaction in kJ/mol?

A coffee-cup calorimeter initially contains 125 g water at 24.2
degrees celsius. Ammonium Nitrate (10.5 g), also at 24.2 degree
celsius, is added to the water, and after the ammonium nitrate
dissolves, the final temperature is 18.3 degrees celsius.What is
the heat of solution of ammonium nitrate in kj/mol? Assume that the
specific heat capacity of the solution is 4.18 J/Cg and that no
heat is transferred to the surrounds or to the calorimeter.

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.

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.

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

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.

A coffee cup calorimeter initially contains 125g of water at
24.2oC. 10.5g of potassium bromide also at
24.2oC is added to the water. After the KBr dissolves
the final temperature is 21.1oC. Calculate the enthalpy
change for dissolving the salt in J/g and kJ/mol. Assume specific
heat of solution is 4.18J/goC.

In the laboratory a "coffee cup" calorimeter, or constant
pressure calorimeter, is frequently used to determine the specific
heat of a solid, or to measure the energy of a solution phase
reaction.
A student heats 60.93 grams of gold to 98.87 °C and then drops it
into a cup containing 79.68 grams of water at 24.46 °C. She
measures the final temperature to be 26.11 °C.
The heat capacity of the calorimeter (sometimes referred to as the
calorimeter constant) was...

A coffee-cup calorimeter containing 100 mL of H2O is used. The
initial temperature of the calorimeter is 23.0 ∘C. If 9.00 g of
CaCl2 is added to the calorimeter, what will be the final
temperature (in ∘C ) of the solution in the calorimeter? The heat
of solution ΔHsoln of CaCl2 is −82.8 kJ/mol.

In the laboratory a student uses a "coffee cup" calorimeter to
determine the specific heat of a metal.
She heats 19.5 grams of tungsten
to 97.80°C and then drops it into a cup containing
78.3 grams of water at 22.58°C.
She measures the final temperature to be
23.20°C.
Assuming that all of the heat is transferred to the water, she
calculates the specific heat of tungsten to
be J/g°C.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 45 minutes ago

asked 46 minutes ago

asked 51 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago