Question

Suppose you have a calorimeter that contains 100.0 grams of water at an initial temperature of 25 degrees celsius. A salt (2.19 g, 0.020 moles) is dissolved in the water, and the final temperature is 29 degrees celsius. Calculate the standard heat of solution (on a per mole basis). Was the dissolution exothermic or endothermic?

Answer #1

There is 300 grams of water in the 200-gram calorimeter cup
(inner can). Both are at room temperature of 20 degrees Celsius. A
100-gram metal sample with an initial temperature of 90 degrees
Celsius is placed in the calorimeter resulting. The resulting final
temperature of the system is 30 degrees Celsius. If the calorimeter
can has a specific heat of 0.2 cal/g-C degree, determine the
specific heat of the metal sample

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

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.

Dissolving 3.00 g of CaCl2(s) in 200.0 g of water in a
calorimeter at 22.4 °C causes the temperature to rise to 25.8 °C.
What is the approximate amount of heat involved in the dissolution,
assuming the heat capacity of the resulting solution is 4.18 J/g
°C? Is the reaction exothermic or endothermic?

A 3.250g sample of methanol, CH3OH, is combusted un a bomb
calorimeter. The temperature of the calorimeter increases by 12.55
degrees celsius. If the heat capacity of the bomb is 850.0
J/degrees celsius and it contains 1.200kg of water, what is the
heat envolved per mole of ethanol combusted? The specific heat
capaacity of water is 4.184 J/g degrees celsius and the molar mass
of methanol is 32.04g/mol.

500 grams of ice at -16 degrees Celsius are dropped into a
calorimeter containing 1000 grams of water at 20 degrees Celsius.
The calorimeter can is of copper and has a mass of 278 grams.
Compute the final temperature of the system, assuming no heat
losses.

A calorimeter contains 75.0 g of water at an initial temperature
of 25.2 °C. 151.28 g of copper metal at a temperature of 95.5 °C
was placed in the calorimeter. The equilibrium temperature was 36.2
°C. The molar heat capacity of water is 75.4 J / mol °C. Determine
the molar heat capacity of the copper.

The aluminum cup inside your calorimeter weighs 40.85 g. You add
49.81 g of water and 3.03 g of KCl to the calorimeter. The initial
temperature is 20.1oC, and the final temperature is 16.9oC. What is
the heat of dissolution for the amounts of salt added, in units of
J? Assume that: the calorimeter is completely insulated the heat
capacity of the empty calorimeter is the heat capacity of the
aluminum cup. the mass of KCl added is small enough...

An insulated aluminum calorimeter vessel of 150 g mass contains
300 g of liquid nitrogen boiling at 77 K. A metal block at an
initial temperature of 303 K is dropped into the liquid nitrogen.
It boils away 15.8 g of nitrogen in reaching thermal equilibrium.
The block is then withdrawn from the nitrogen and quickly
transferred to a second insulated copper calorimeter vessel of 200
g mass containing 500 g of water at 30.1 degrees celsius. The block
coolds...

A.The heat change in a chemical reaction at constant
_____________ is quantitatively expressed as the change of the
enthalpy for the reaction.
temperature
volume
pressure
amount of mole
B.What will be final temperature if you mix the 50.g of water at
0.0oC to 50.g of water at 100.0oC.
75.0 degree Celsius
20.0 degree Celsius
90.0 degree Celsius
50.0 degree Celsius
C.Which will be the range of final temperature, Tfinal (oC) if
you mix the 50.g of Magnesium metal (S=1.020 J/goC)...

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