Question
In: Chemistry
In the following experiment, a coffee-cup calorimeter containing 100 mL of H2O is used. The initial...
In the following experiment, a coffee-cup calorimeter containing 100 mL of H2O is used. The initial temperature of the calorimeter is 23.0 ∘C. If 8.50 g of CaCl2 is added to the calorimeter, what will be the final temperature of the solution in the calorimeter? The heat of solution ΔHsoln of CaCl2 is −82.8 kJ/mol.
Express your answer with the appropriate units.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
In the following experiment, a coffee-cup calorimeter containing 100 mL of H2O is used. The initial...
In the following experiment, a coffee-cup calorimeter containing
100 mL of H2O is used. The initial temperature of the calorimeter
is 23.0 ∘C. If 7.10 g of CaCl2 is added to the calorimeter, what
will be the final temperature of the solution in the calorimeter?
The heat of solution ΔHsoln of CaCl2 is −82.8 kJ/mol.
Express your answer with the appropriate units.
In the following experiment, a coffee-cup calorimeter containing 100 mL of H2O is used. The initial...
In the following experiment, a coffee-cup calorimeter containing
100 mL of H2O is used. The initial temperature of the calorimeter
is 23.0 ∘C. If 4.90 g of CaCl2 is added to the calorimeter, what
will be the final temperature of the solution in the calorimeter?
The heat of solution ΔHsoln of CaCl2 is −82.8 kJ/mol.
Part A In the following experiment, a coffee-cup calorimeter containing 100 mL of H2O is used....
Part A
In the following experiment, a coffee-cup calorimeter containing
100 mL of H2O is used. The initial temperature of the calorimeter
is 23.0 ∘C. If 4.00 g of CaCl2 is added to the calorimeter, what
will be the final temperature of the solution in the calorimeter?
The heat of solution ΔHsoln of CaCl2 is −82.8 kJ/mol.
Express your answer with the appropriate units.
Hints
In a coffee-cup calorimeter experiment, if we ignored the heat lost to the Styrofoam cup and...
In a coffee-cup calorimeter experiment, if we ignored the heat
lost to the Styrofoam cup and the air, does this cause the heat
gained by the total solution at the end to be too big or too small.
Could you please explain.
In the laboratory a"coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the...
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 heats65.62grams ofzincto98.24 °C and then drops
it into a cup containing75.87grams of water at23.87 °C. She
measures the final temperature to be29.24 °C. The heat capacity of
the calorimeter (sometimes referred to as thecalorimeter constant)
was determined in a separate experiment to be1.54J/°C. Assuming
that no heat...
A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in an unknown...
A coffee-cup (constant pressure) calorimeter is used to carry
out the following reaction in an unknown volume of water (where X
is a hypothetical metal): X + 2 H2O → X(OH)2 + H2 In this process,
the water temperature rose from 25.0 °C to 32.2 °C. If 0.00803 mol
of "X" was consumed during the reaction, and the ΔH of this
reaction with respect to the system is -1798 kJ mol-1 , what volume
of water (in mL) was present...
50 mL of .500 M NaOH is placed in a coffee-cup calorimeter at 25.00 degreees Celsius...
50 mL of .500 M NaOH is placed in a coffee-cup
calorimeter at 25.00 degreees Celsius and 25 mL of .250 M H2SO4 is
carefully added, also at 25.00 degrees Celsius. After stirring the
final temperature is 27.21 degrees Celsius. Calculate q (soln) in J
and the change in enthalpy, delta h in kj/mol of H2O formed. Assume
that the total volume is the sum of the individual volumes, that
d=1.00 g/mL, and that c= 4.184 J/g-k.
You place 59.7 ml of 0.605 M NaOH in a coffee- cup calorimeter at 25.00°C and...
You place 59.7 ml of 0.605 M NaOH in a coffee- cup calorimeter
at 25.00°C and add 76 ml of 0.605 M HCl, also at 25.00°C. After
stirring, the final temperature is 27.84°C. [Assume the total
volume is the sum of the individual volumes and that the final
solution has the same density (1.00 g/ml) and specific heat
capacity (4.184 J/gK)]. Calculate the change in enthalpy of the
reaction in kJ/mol of water formed. Enter to 1 decimal place. Hint:...
You place 41.8 ml of 0.541 M NaOH in a coffee- cup calorimeter at 25.00°C and...
You place 41.8 ml of 0.541 M NaOH in a coffee- cup calorimeter
at 25.00°C and add 73.3 ml of 0.541 M HCl, also at 25.00°C. After
stirring, the final temperature is 28.24°C. [Assume the total
volume is the sum of the individual volumes and that the final
solution has the same density (1.00 g/ml) and specific heat
capacity (4.184 J/gK)]. Calculate the change in enthalpy (LaTeX:
\DeltaΔH) of the reaction in kJ/mol of water formed. Enter to 1
decimal...
Steam at 100°C is condensed into a 54.0 g aluminum calorimeter cup containing 260 g of...
Steam at 100°C is condensed into a 54.0 g aluminum calorimeter
cup containing 260 g of water at 25.0°C. Determine the amount of
steam (in g) needed for the system to reach a final temperature of
64.0°C. The specific heat of aluminum is 900 J/(kg · °C).
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