Question

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

Answer #1

Total volume = 23.8 mL + 23.8 mL = 47.6 mL

Density of the solution = 1 g/mL (Assumed same as that of water)

Therefore, mass of the solution = Volume x Density = 47.6 g

Heat gained by the calori meter, q_{reaction} = mcT =
47.6 g x 4.184 J/goC x (30.17- 23.50) = 1328.4 J

Heat released during the reaction, q_{neutralization} =
-1328.4 J

Moles of H_{2}SO_{4} used = 0.5 M x (0.0238 L) =
0.0119 moles

Moles of KOH used = 1 M x (0.0238 L) = 0.0238 moles

H_{2}SO_{4} + 2KOH
K_{2}SO_{4} + 2H_{2}O

Thus, one mole of H_{2}SO_{4} produces two moles
of H_{2}O

Therefore, 0.0119 moles of H_{2}SO_{4} will
produce 0.0119 x 2 = 0.0238 moles of H_{2}O

Similarly, 0.0238 moles of KOH will produce 0.0238 moles of
H_{2}O

Therefore,

H =
-q_{neutralization}/ Moles of H_{2}O = -1328.4 J/
0.0238 = -55.8 kJ/mol

**Enthalpy of the reaction = -55.8 kJ/mol**

When 26.5 mL of 0.500 M
H2SO4 is added to 26.5 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).
Answer in kJ/molH2O

When 27.7 mL of 0.500 M H2SO4 is added to 27.7 mL of 1.00 M KOH
in a coffee-cup calorimeter at 23.50°C, the temperature rises to
30.17°C. Calculate ?H 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.)

When 26.6 mL of 0.500 M
H2SO4
is added to 26.6 mL of 1.00 M KOH
in a coffee-cup calorimeter at 23.50
°
C, the temperature rises to 30.17
°
C. Calculate
Δ
H 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
·...

Enter your answer in the provided box.
When 22.9 mL of 0.500 M H2SO4 is
added to 22.9 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 =...

When 30.5 mL of 0.515 M H2SO4 is added to 30.5 mL of 1.03 M KOH
in a coffee-cup calorimeter at 23.50°C, the temperature rises to
30.17°C. Calculate H of this reaction per mole of H2SO4 and KOH
reacted. (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 = 1.00 g/mL and c =
4.184 J/g×K.)

In a constant-pressure calorimeter, 50.0 mL of 0.930 M H2SO4 was
added to 50.0 mL of 0.290 M NaOH. The reaction caused the
temperature of the solution to rise from 21.88 °C to 23.86 °C. If
the solution has the same density and specific heat as water (1.00
g/mL and 4.184 J/g·K, respectively), what is ΔH for this reaction
(per mole of H2O produced)? Assume that the total volume is the sum
of the individual volumes.

In a constant-pressure calorimeter, 55.0 mL of 0.840 M H2SO4 was
added to 55.0 mL of 0.260 M NaOH. The reaction caused the
temperature of the solution to rise from 21.91 °C to 23.68 °C. If
the solution has the same density and specific heat as water (1.00
g/mL and 4.184 J/g·K, respectively), what is ΔH for this reaction
(per mole of H2O produced)? Assume that the total volume is the sum
of the individual volumes.

50.0 mL of 0.100 M KOH, at 20.00o C, is added to
50.00 mL of 0.110 M HCl, at 20.00o C, in a coffee cup
calorimeter. The enthalpy of neutralization is 56.0 kJ/mol. The
specific heat capacity of the total solution is 4.184 Jg-1
oC-1, and the density of the total
solution is 1.00 g/mL, what is Tf for the reaction?

300 mL of a 0.694 M HCl aqueous solution is mixed with 300 mL of
0.347 M Ba(OH)2 aqueous solution in a coffee-cup calorimeter. Both
the solutions have an initial temperature of 28.7 °C. Calculate the
final temperature of the resulting solution, given the following
information:
H+(aq) + OH- (aq) ? H2O(?) ? ? ? ?Hrxn = -56.2 kJ/mol
Assume that volumes can be added, that the density of the solution
is the same as that of water (1.00 g/mL),...

You place 40.3 ml of 0.366 M NaOH in a coffee- cup calorimeter
at 25.00°C and add 64.8 ml of 0.366 M HCl, also at 25.00°C. After
stirring, the final temperature is 27.93°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 (ΔH) of
the reaction in kJ/mol of water formed. Enter to 1 decimal place....

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 2 minutes ago

asked 7 minutes ago

asked 7 minutes ago

asked 10 minutes ago

asked 10 minutes ago

asked 13 minutes ago

asked 13 minutes ago

asked 13 minutes ago

asked 21 minutes ago

asked 21 minutes ago

asked 25 minutes ago

asked 25 minutes ago