Question

Given the data in the table below, what is the enthalpy of dissolution of KOH? The molar mass of KOH is 56.11 g/mol, the specific heat of solution is 4.184 J/gºC, and the calorimeter constant is 22.45 J/ºC. To receive full points for this question, list every step of your calculation.

mass of water added to the calorimeter 50.000 g

initial temperature of the water 22.0 ºC

mass of KOH added to the calorimeter 1.824 g

final temperature in the calorimeter 29.9 ºC

Answer #1

In an experiment to determine the enthalpy of fusion of ice, the
following data was collected:
Initial mass of water in the calorimeter = 70.89g
Initial temperature of the water in the calorimeter = 17.6
degrees C
Final mass of temperature in the calorimeter = 0.0 degrees C
Please calculate:
a) the mass of the ice that melted
b) the number of mol of ice that melted
c) the change in temperature of the initial mass of water in the...

When 23.8 mL of 0.500 M H2SO4 is added to 23.8 mL of 1.00 M KOH
in a coffee-cup calorimeter at 23.50°C, the temperature rises to
30.17°C. Calculate ΔH of this reaction. (Assume that the total
volume is the sum of the individual volumes and that the density
and specific heat capacity of the solution are the same as for pure
water.) (d for water = 1.00 g/mL; c for water = 4.184 J/g·°C.)
?: kJ/mol H2O

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.

1.
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
6.20 g of CsClO4(s)
are dissolved in 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 CsClO4(s) in
kJ/mol.
Assume the specific heat of the solution is...

Part A A calorimeter contains 25.0 mL of water at 11.5 ∘ C .
When 1.20 g of X (a substance with a molar mass of 73.0 g/mol ) is
added, it dissolves via the reaction X(s)+ H 2 O(l)→X(aq) and the
temperature of the solution increases to 30.0 ∘ C . Calculate the
enthalpy change, ΔH , for this reaction per mole of X . Assume that
the specific heat of the resulting solution is equal to that of...

When 1.020 g of ethanol (C2H6O, 46.07 g/mol) was burned in a
bomb calorimeter containing 2400. g of water, the temperature of
the water rose from 22.46 to 25.52ºC. The specific heat
of water is 4.18 J/g-°C. What is the enthalpy of combustion of 1
mol of ethanol? What is the heat capacity of the calorimeter?

A 1.000 kg block of ice at 0 °C is dropped into 1.354 kg of
water that is 45 °C. What mass of ice melts?
Specific heat of ice = 2.092 J/(g*K) Water = 4.184
J/(g*K) Steam = 1.841 J/(g*K) Enthalpy of fusion =
6.008 kJ/mol Enthalpy of vaporization = 40.67 kJ/mol

1. A 78.0 g piece of metal at 89.0°C is placed in 125 g of water
at 21.0°C contained in a calorimeter. The metal and water come to
the same temperature at 27.0°C.
- How much heat (in J) did the metal give up to the water?
(Assume the specific heat of water is 4.18 J/g·°C across the
temperature range.)
- What is the specific heat (in J/g·°C) of the metal?
2. A 0.529 g sample of KCl is added...

A calorimeter is an insulated device in which a chemical
reaction is contained. By measuring the temperature change, ΔT, we
can calculate the heat released or absorbed during the reaction
using the following equation: q=specific heat×mass×ΔT Or, if the
calorimeter has a predetermined heat capacity, C, the equation
becomes q=C×ΔT At constant pressure, the enthalpy change for the
reaction, ΔH, is equal to the heat, qp; that is, ΔH=qp but it is
usually expressed per mole of reactant and with...

When pure sulfuric acid dissolves in water, much heat is given
off. To measure it, 4.90 g sulfuric acid is added to 175 g water,
both at 10.0 ºC in coffee-cup calorimeter. The temperature of the
mixture rose to 14.9 ºC. Assuming no heat loss and the density and
the specific heat of the solution to be the same as that of water,
calculate the heat evolved per mole of sulfuric acid.

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