Question

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.

Answer #1

total gm of soution = 125 + 10.5 = 135.5 gm

T = 24.2 - 18.3 =
5.9^{0}C

q = mass of solution specific heat of T

= 135.5 4.18 5.9

q = 3341.701 J = 3.3417 KJ

molar mass of ammonium nitrate = 80.043 gm/mol

then 10 .5 gm of ammonium nitrate = 10.5/80.043 = 0.1311 mole

0.1311 mole of ammonium nitrate have heat of solution 3.3417 KJ then 1 mole of ammonium nitrate have heat of solution = 1 3.3417 / 0.1311 = 25.4897 KJ

Heat of solution of ammonium nitrate is = 25.4897 KJ/mol

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.

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.

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

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 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?

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 9.07-g sample of NaOH is dissolved in 104.9 g of water in a
coffee cup calorimeter. The temperature of the solution rises from
15.49°C to 23.76°C. Calculate ∆Hrxn,
in kJ for the dissociation of NaOH in water Assume that the heat
capacity for the solution is 4.18 J/g°C.

a 25.0g piece of aluminum (molar heat capacity of 24.03 J/g
degrees Celsius) is heated to 82.4 degrees Celsius and dropped into
a calorimeter containing water (specific heat capacity of water is
4.18 J/g degrees Celsius) initially at 22.3 degrees Celsius. The
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A coffee-cup calorimeter contains 130.0 g of water at 25.3 ∘C .
A 124.0-g block of copper metal is heated to 100.4 ∘C by putting it
in a beaker of boiling water. The specific heat of Cu(s) is 0.385
J/g⋅K . The Cu is added to the calorimeter, and after a time the
contents of the cup reach a constant temperature of 30.3 ∘C .
Part A
Determine the amount of heat, in J , lost by the copper block....

1. What is the final temperature of a solution initially at 22.0
celsius if 2.45 g of a solid is dropped into 34.5 g of the solution
resulting in the reaction between the two that absorbs 1350 J of
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2. If a 31.25g piece of an unknown metal at 25 Celsius was added
to 25.0 g of water at 100.0Celsius and the two equilibrated at 95.2
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3. In...

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